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5 Apr 2023

16 pages

Learn How to Calculate Empirical and Molecular Formulas for Different Compounds

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JJ

@jjstudymaster

Understanding empirical formulas and molecular formulasis fundamental to mastering... Show more

2.4 Empirical and Molecular
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Understanding Empirical and Molecular Formulas in Chemistry

The empirical formula represents the simplest whole number ratio of atoms in a compound, while the molecular formula shows the actual number of atoms present. Understanding how to calculate these formulas is crucial for chemical analysis and compound identification.

Definition: An empirical formula shows the simplest whole-number ratio of atoms in a compound, while a molecular formula shows the actual number of atoms present in one molecule.

When determining empirical formulas, chemists follow a systematic process involving mass measurements and molar calculations. For example, when finding the empirical formula of calcium carbonate, we first measure the mass of each element, convert to moles, and then find the simplest whole number ratio.

The relationship between empirical and molecular formulas becomes clear when working with compounds like glucose C6H12O6C6H12O6. While its empirical formula is CH2O, the molecular formula is six times larger, showing that molecular formulas are always whole number multiples of empirical formulas.

2.4 Empirical and Molecular
Formula
Notes
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00
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Calculating Empirical Formulas from Experimental Data

When working with metal oxides like copperIIII oxide, determining empirical formulas often involves reduction experiments. The process requires careful mass measurements before and after reduction to calculate the oxygen content.

Example: To find the empirical formula of copper oxide, if 0.795g of black copper oxide reduces to 0.635g of copper, the mass difference of 0.160g represents oxygen. Converting these masses to moles gives a 1:1 ratio, resulting in CuO.

Other common metal oxides follow similar patterns:

  • Iron IIIIII oxide formula: Fe2O3
  • Aluminum oxide formula: Al2O3
  • Magnesium oxide formula: MgO

Highlight: Metal oxides are particularly important in industry and serve as excellent examples for teaching empirical formula calculations.

2.4 Empirical and Molecular
Formula
Notes
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Covered in Class Done
To-Do List:
00
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Advanced Formula Determination Methods

Learning how to find molecular formula from empirical formula requires understanding the relationship between molar mass and empirical formula mass. The process involves:

  1. Calculating the empirical formula mass
  2. Determining the actual molar mass
  3. Finding the multiplication factor between them

Vocabulary: The empirical formula mass is the sum of the atomic masses of all atoms in the empirical formula, while molar mass represents the mass of one mole of the actual molecule.

Students practicing how to find empirical formula with percentages must convert percentage composition to masses, then follow the standard procedure of converting to moles and finding ratios.

2.4 Empirical and Molecular
Formula
Notes
Anki
Covered in Class Done
To-Do List:
00
Add and Use Specification Reference
Add class Notes
add

Practical Applications and Problem-Solving Strategies

When working with empirical and molecular formula practice problems, students should develop a systematic approach. This includes:

  1. Converting given data to masses
  2. Calculating moles of each element
  3. Finding the simplest whole number ratio
  4. Determining any multiplication factor needed for molecular formulas

Example: For cyclohexane C6H12C6H12, if analysis shows 55.56g carbon and 9.29g hydrogen, converting to moles gives a 1:2 ratio CH2CH2 as the empirical formula. The molecular formula is determined by comparing this to the actual molar mass.

Understanding how to calculate empirical formula mass is essential for connecting empirical and molecular formulas in real-world applications. This skill is particularly important in organic chemistry and industrial chemical analysis.

2.4 Empirical and Molecular
Formula
Notes
Anki
Covered in Class Done
To-Do List:
00
Add and Use Specification Reference
Add class Notes
add

Understanding Empirical and Molecular Formulas in Chemistry

The process of determining empirical and molecular formulas is fundamental in chemistry analysis. When working with chemical compounds, understanding how to calculate these formulas helps identify the basic composition and structure of substances.

Definition: An empirical formula shows the simplest whole-number ratio of atoms in a compound, while a molecular formula shows the actual number of atoms present in one molecule.

Let's examine how to find the empirical formula using percentage composition. Consider a compound containing 55.56 grams of carbon and 9.29 grams of hydrogen. To determine the empirical formula, we first convert masses to moles by dividing each mass by its atomic mass. For carbon, dividing 55.56 by 12.01 gives 4.63 moles. For hydrogen, dividing 9.29 by 1.008 gives 9.29 moles. The ratio becomes 4.63:9.29, which simplifies to 1:2, giving us CH₂.

Example: When working with percentages, like in a compound containing 31.6% carbon, 5.3% hydrogen, and 63.1% oxygen, convert each percentage to moles first. Divide each percentage by the respective atomic mass, then find the simplest whole-number ratio.

2.4 Empirical and Molecular
Formula
Notes
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Covered in Class Done
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00
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Converting Between Empirical and Molecular Formulas

Understanding how to find molecular formula from empirical formula requires knowing the compound's molar mass. The relationship between empirical and molecular formulas is crucial for chemical analysis.

Highlight: The molecular formula is always a whole-number multiple of the empirical formula. To find it, divide the molecular mass by the empirical formula mass.

For example, when analyzing a compound containing 43.66% phosphorus and 56.34% oxygen with a molecular mass of 284 g/mol, first determine the empirical formula. Converting percentages to moles gives P₂O₅ as the empirical formula. The empirical formula mass is 142 g/mol. Dividing 284 by 142 gives 2, meaning the molecular formula is P2O5P₂O₅₂ or P₄O₁₀.

Vocabulary: The empirical formula mass is the sum of the atomic masses of all atoms shown in the empirical formula.

2.4 Empirical and Molecular
Formula
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Analyzing Metal Oxides and Their Formulas

Understanding metal oxide formulas is essential in inorganic chemistry. Common examples include iron IIIIII oxide formula Fe2O3Fe₂O₃, aluminum oxide formula Al2O3Al₂O₃, and magnesium oxide formula MgOMgO.

Example: To determine the empirical formula of copper oxide, conduct a reduction experiment where copperIIII oxide blackblack is reduced to copper metal reddishbrownreddish-brown. The mass difference reveals the oxygen content.

The color change from black to reddish-brown in copper oxide reduction serves as a visual indicator of the reaction's progress. This practical application helps students understand oxidation states and chemical reactions while determining empirical formulas.

2.4 Empirical and Molecular
Formula
Notes
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Covered in Class Done
To-Do List:
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Practice and Applications in Formula Determination

To master how to find empirical formula with percentages, regular practice with various compounds is essential. Students should work through problems involving both simple and complex molecules.

Definition: The empirical formula mass is calculated by adding the atomic masses of all elements in their empirical formula ratios.

When solving problems involving molecular formula from empirical formula and molar mass, follow these steps:

  1. Calculate the empirical formula using percentage or mass data
  2. Determine the empirical formula mass
  3. Divide the molecular mass by the empirical formula mass
  4. Multiply the empirical formula by this number

Example: For CaCO₃ molecular formula, the empirical and molecular formulas are identical because the simplest ratio represents the actual molecule.

2.4 Empirical and Molecular
Formula
Notes
Anki
Covered in Class Done
To-Do List:
00
Add and Use Specification Reference
Add class Notes
add

Understanding Empirical and Molecular Formulas in Chemistry

The relationship between empirical and molecular formulas plays a crucial role in determining chemical compositions. When analyzing compounds, chemists must understand how to convert between these two fundamental representations of molecular structure.

Definition: An empirical formula shows the simplest whole-number ratio of atoms in a compound, while a molecular formula shows the actual number of atoms present in one molecule.

Consider a practical example of finding both formulas for a compound containing 40.0% carbon, 6.7% hydrogen, and 53.3% oxygen with a molecular mass of 180 g/mol. To solve this, we must first determine the empirical formula by converting percentages to moles:

For carbon: 40.0% ÷ 12.0 = 3.33 moles For hydrogen: 6.7% ÷ 1.0 = 6.7 moles For oxygen: 53.3% ÷ 16.0 = 3.33 moles

Example: After finding the mole ratios, divide all values by the smallest number to get the simplest whole-number ratio. In this case, the empirical formula would be CH2O, as the ratio becomes 1:2:1.

The molecular formula can then be determined by comparing the empirical formula mass to the actual molecular mass. If the molecular mass is a multiple of the empirical formula mass, multiply the subscripts in the empirical formula by this factor to obtain the molecular formula.

2.4 Empirical and Molecular
Formula
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Advanced Applications of Molecular Formula Calculations

Understanding how to find molecular formulas from empirical formulas extends beyond basic calculations. This knowledge is essential when working with various metal oxides and complex organic compounds.

Highlight: Metal oxides like iron IIIIII oxide formula Fe2O3Fe2O3, aluminum oxide formula Al2O3Al2O3, and magnesium oxide formula MgOMgO demonstrate how empirical formulas can also be molecular formulas in some cases.

The transformation from empirical to molecular formula becomes particularly important when dealing with larger molecules. For instance, glucose C6H12O6C6H12O6 has an empirical formula of CH2O, but its molecular formula reveals the actual structure containing six times as many atoms.

Vocabulary: The relationship between empirical and molecular formulas can be expressed as: Molecular Formula = EmpiricalFormulaEmpirical Formulan, where n is a whole number.

When working with copperIIII oxide, its characteristic black color and chemical behavior help verify the empirical formula determined through laboratory analysis. This practical application demonstrates how physical properties can support theoretical calculations in determining molecular structures.



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The app is very easy to use and well designed. I have found everything I was looking for so far and have been able to learn a lot from the presentations! I will definitely use the app for a class assignment! And of course it also helps a lot as an inspiration.

Stefan S

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This app is really great. There are so many study notes and help [...]. My problem subject is French, for example, and the app has so many options for help. Thanks to this app, I have improved my French. I would recommend it to anyone.

Samantha Klich

Android user

Wow, I am really amazed. I just tried the app because I've seen it advertised many times and was absolutely stunned. This app is THE HELP you want for school and above all, it offers so many things, such as workouts and fact sheets, which have been VERY helpful to me personally.

Anna

iOS user

Best app on earth! no words because it’s too good

Thomas R

iOS user

Just amazing. Let's me revise 10x better, this app is a quick 10/10. I highly recommend it to anyone. I can watch and search for notes. I can save them in the subject folder. I can revise it any time when I come back. If you haven't tried this app, you're really missing out.

Basil

Android user

This app has made me feel so much more confident in my exam prep, not only through boosting my own self confidence through the features that allow you to connect with others and feel less alone, but also through the way the app itself is centred around making you feel better. It is easy to navigate, fun to use, and helpful to anyone struggling in absolutely any way.

David K

iOS user

The app's just great! All I have to do is enter the topic in the search bar and I get the response real fast. I don't have to watch 10 YouTube videos to understand something, so I'm saving my time. Highly recommended!

Sudenaz Ocak

Android user

In school I was really bad at maths but thanks to the app, I am doing better now. I am so grateful that you made the app.

Greenlight Bonnie

Android user

very reliable app to help and grow your ideas of Maths, English and other related topics in your works. please use this app if your struggling in areas, this app is key for that. wish I'd of done a review before. and it's also free so don't worry about that.

Rohan U

Android user

I know a lot of apps use fake accounts to boost their reviews but this app deserves it all. Originally I was getting 4 in my English exams and this time I got a grade 7. I didn’t even know about this app three days until the exam and it has helped A LOT. Please actually trust me and use it as I’m sure you too will see developments.

Xander S

iOS user

THE QUIZES AND FLASHCARDS ARE SO USEFUL AND I LOVE THE SCHOOLGPT. IT ALSO IS LITREALLY LIKE CHATGPT BUT SMARTER!! HELPED ME WITH MY MASCARA PROBLEMS TOO!! AS WELL AS MY REAL SUBJECTS ! DUHHH 😍😁😲🤑💗✨🎀😮

Elisha

iOS user

This apps acc the goat. I find revision so boring but this app makes it so easy to organize it all and then you can ask the freeeee ai to test yourself so good and you can easily upload your own stuff. highly recommend as someone taking mocks now

Paul T

iOS user

 

Chemistry

286

5 Apr 2023

16 pages

Learn How to Calculate Empirical and Molecular Formulas for Different Compounds

user profile picture

JJ

@jjstudymaster

Understanding empirical formulas and molecular formulas is fundamental to mastering chemical composition calculations in chemistry.

The empirical formula represents the simplest whole-number ratio of atoms in a compound, while the molecular formulashows the actual number of atoms present. For... Show more

2.4 Empirical and Molecular
Formula
Notes
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Understanding Empirical and Molecular Formulas in Chemistry

The empirical formula represents the simplest whole number ratio of atoms in a compound, while the molecular formula shows the actual number of atoms present. Understanding how to calculate these formulas is crucial for chemical analysis and compound identification.

Definition: An empirical formula shows the simplest whole-number ratio of atoms in a compound, while a molecular formula shows the actual number of atoms present in one molecule.

When determining empirical formulas, chemists follow a systematic process involving mass measurements and molar calculations. For example, when finding the empirical formula of calcium carbonate, we first measure the mass of each element, convert to moles, and then find the simplest whole number ratio.

The relationship between empirical and molecular formulas becomes clear when working with compounds like glucose C6H12O6C6H12O6. While its empirical formula is CH2O, the molecular formula is six times larger, showing that molecular formulas are always whole number multiples of empirical formulas.

2.4 Empirical and Molecular
Formula
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Calculating Empirical Formulas from Experimental Data

When working with metal oxides like copperIIII oxide, determining empirical formulas often involves reduction experiments. The process requires careful mass measurements before and after reduction to calculate the oxygen content.

Example: To find the empirical formula of copper oxide, if 0.795g of black copper oxide reduces to 0.635g of copper, the mass difference of 0.160g represents oxygen. Converting these masses to moles gives a 1:1 ratio, resulting in CuO.

Other common metal oxides follow similar patterns:

  • Iron IIIIII oxide formula: Fe2O3
  • Aluminum oxide formula: Al2O3
  • Magnesium oxide formula: MgO

Highlight: Metal oxides are particularly important in industry and serve as excellent examples for teaching empirical formula calculations.

2.4 Empirical and Molecular
Formula
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Advanced Formula Determination Methods

Learning how to find molecular formula from empirical formula requires understanding the relationship between molar mass and empirical formula mass. The process involves:

  1. Calculating the empirical formula mass
  2. Determining the actual molar mass
  3. Finding the multiplication factor between them

Vocabulary: The empirical formula mass is the sum of the atomic masses of all atoms in the empirical formula, while molar mass represents the mass of one mole of the actual molecule.

Students practicing how to find empirical formula with percentages must convert percentage composition to masses, then follow the standard procedure of converting to moles and finding ratios.

2.4 Empirical and Molecular
Formula
Notes
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Practical Applications and Problem-Solving Strategies

When working with empirical and molecular formula practice problems, students should develop a systematic approach. This includes:

  1. Converting given data to masses
  2. Calculating moles of each element
  3. Finding the simplest whole number ratio
  4. Determining any multiplication factor needed for molecular formulas

Example: For cyclohexane C6H12C6H12, if analysis shows 55.56g carbon and 9.29g hydrogen, converting to moles gives a 1:2 ratio CH2CH2 as the empirical formula. The molecular formula is determined by comparing this to the actual molar mass.

Understanding how to calculate empirical formula mass is essential for connecting empirical and molecular formulas in real-world applications. This skill is particularly important in organic chemistry and industrial chemical analysis.

2.4 Empirical and Molecular
Formula
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Understanding Empirical and Molecular Formulas in Chemistry

The process of determining empirical and molecular formulas is fundamental in chemistry analysis. When working with chemical compounds, understanding how to calculate these formulas helps identify the basic composition and structure of substances.

Definition: An empirical formula shows the simplest whole-number ratio of atoms in a compound, while a molecular formula shows the actual number of atoms present in one molecule.

Let's examine how to find the empirical formula using percentage composition. Consider a compound containing 55.56 grams of carbon and 9.29 grams of hydrogen. To determine the empirical formula, we first convert masses to moles by dividing each mass by its atomic mass. For carbon, dividing 55.56 by 12.01 gives 4.63 moles. For hydrogen, dividing 9.29 by 1.008 gives 9.29 moles. The ratio becomes 4.63:9.29, which simplifies to 1:2, giving us CH₂.

Example: When working with percentages, like in a compound containing 31.6% carbon, 5.3% hydrogen, and 63.1% oxygen, convert each percentage to moles first. Divide each percentage by the respective atomic mass, then find the simplest whole-number ratio.

2.4 Empirical and Molecular
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Converting Between Empirical and Molecular Formulas

Understanding how to find molecular formula from empirical formula requires knowing the compound's molar mass. The relationship between empirical and molecular formulas is crucial for chemical analysis.

Highlight: The molecular formula is always a whole-number multiple of the empirical formula. To find it, divide the molecular mass by the empirical formula mass.

For example, when analyzing a compound containing 43.66% phosphorus and 56.34% oxygen with a molecular mass of 284 g/mol, first determine the empirical formula. Converting percentages to moles gives P₂O₅ as the empirical formula. The empirical formula mass is 142 g/mol. Dividing 284 by 142 gives 2, meaning the molecular formula is P2O5P₂O₅₂ or P₄O₁₀.

Vocabulary: The empirical formula mass is the sum of the atomic masses of all atoms shown in the empirical formula.

2.4 Empirical and Molecular
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Analyzing Metal Oxides and Their Formulas

Understanding metal oxide formulas is essential in inorganic chemistry. Common examples include iron IIIIII oxide formula Fe2O3Fe₂O₃, aluminum oxide formula Al2O3Al₂O₃, and magnesium oxide formula MgOMgO.

Example: To determine the empirical formula of copper oxide, conduct a reduction experiment where copperIIII oxide blackblack is reduced to copper metal reddishbrownreddish-brown. The mass difference reveals the oxygen content.

The color change from black to reddish-brown in copper oxide reduction serves as a visual indicator of the reaction's progress. This practical application helps students understand oxidation states and chemical reactions while determining empirical formulas.

2.4 Empirical and Molecular
Formula
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Practice and Applications in Formula Determination

To master how to find empirical formula with percentages, regular practice with various compounds is essential. Students should work through problems involving both simple and complex molecules.

Definition: The empirical formula mass is calculated by adding the atomic masses of all elements in their empirical formula ratios.

When solving problems involving molecular formula from empirical formula and molar mass, follow these steps:

  1. Calculate the empirical formula using percentage or mass data
  2. Determine the empirical formula mass
  3. Divide the molecular mass by the empirical formula mass
  4. Multiply the empirical formula by this number

Example: For CaCO₃ molecular formula, the empirical and molecular formulas are identical because the simplest ratio represents the actual molecule.

2.4 Empirical and Molecular
Formula
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Understanding Empirical and Molecular Formulas in Chemistry

The relationship between empirical and molecular formulas plays a crucial role in determining chemical compositions. When analyzing compounds, chemists must understand how to convert between these two fundamental representations of molecular structure.

Definition: An empirical formula shows the simplest whole-number ratio of atoms in a compound, while a molecular formula shows the actual number of atoms present in one molecule.

Consider a practical example of finding both formulas for a compound containing 40.0% carbon, 6.7% hydrogen, and 53.3% oxygen with a molecular mass of 180 g/mol. To solve this, we must first determine the empirical formula by converting percentages to moles:

For carbon: 40.0% ÷ 12.0 = 3.33 moles For hydrogen: 6.7% ÷ 1.0 = 6.7 moles For oxygen: 53.3% ÷ 16.0 = 3.33 moles

Example: After finding the mole ratios, divide all values by the smallest number to get the simplest whole-number ratio. In this case, the empirical formula would be CH2O, as the ratio becomes 1:2:1.

The molecular formula can then be determined by comparing the empirical formula mass to the actual molecular mass. If the molecular mass is a multiple of the empirical formula mass, multiply the subscripts in the empirical formula by this factor to obtain the molecular formula.

2.4 Empirical and Molecular
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Advanced Applications of Molecular Formula Calculations

Understanding how to find molecular formulas from empirical formulas extends beyond basic calculations. This knowledge is essential when working with various metal oxides and complex organic compounds.

Highlight: Metal oxides like iron IIIIII oxide formula Fe2O3Fe2O3, aluminum oxide formula Al2O3Al2O3, and magnesium oxide formula MgOMgO demonstrate how empirical formulas can also be molecular formulas in some cases.

The transformation from empirical to molecular formula becomes particularly important when dealing with larger molecules. For instance, glucose C6H12O6C6H12O6 has an empirical formula of CH2O, but its molecular formula reveals the actual structure containing six times as many atoms.

Vocabulary: The relationship between empirical and molecular formulas can be expressed as: Molecular Formula = EmpiricalFormulaEmpirical Formulan, where n is a whole number.

When working with copperIIII oxide, its characteristic black color and chemical behavior help verify the empirical formula determined through laboratory analysis. This practical application demonstrates how physical properties can support theoretical calculations in determining molecular structures.

Similar content

A level chemistry definitions

930

30

Can't find what you're looking for? Explore other subjects.

Students love us — and so will you.

4.9/5

App Store

4.8/5

Google Play

The app is very easy to use and well designed. I have found everything I was looking for so far and have been able to learn a lot from the presentations! I will definitely use the app for a class assignment! And of course it also helps a lot as an inspiration.

Stefan S

iOS user

This app is really great. There are so many study notes and help [...]. My problem subject is French, for example, and the app has so many options for help. Thanks to this app, I have improved my French. I would recommend it to anyone.

Samantha Klich

Android user

Wow, I am really amazed. I just tried the app because I've seen it advertised many times and was absolutely stunned. This app is THE HELP you want for school and above all, it offers so many things, such as workouts and fact sheets, which have been VERY helpful to me personally.

Anna

iOS user

Best app on earth! no words because it’s too good

Thomas R

iOS user

Just amazing. Let's me revise 10x better, this app is a quick 10/10. I highly recommend it to anyone. I can watch and search for notes. I can save them in the subject folder. I can revise it any time when I come back. If you haven't tried this app, you're really missing out.

Basil

Android user

This app has made me feel so much more confident in my exam prep, not only through boosting my own self confidence through the features that allow you to connect with others and feel less alone, but also through the way the app itself is centred around making you feel better. It is easy to navigate, fun to use, and helpful to anyone struggling in absolutely any way.

David K

iOS user

The app's just great! All I have to do is enter the topic in the search bar and I get the response real fast. I don't have to watch 10 YouTube videos to understand something, so I'm saving my time. Highly recommended!

Sudenaz Ocak

Android user

In school I was really bad at maths but thanks to the app, I am doing better now. I am so grateful that you made the app.

Greenlight Bonnie

Android user

very reliable app to help and grow your ideas of Maths, English and other related topics in your works. please use this app if your struggling in areas, this app is key for that. wish I'd of done a review before. and it's also free so don't worry about that.

Rohan U

Android user

I know a lot of apps use fake accounts to boost their reviews but this app deserves it all. Originally I was getting 4 in my English exams and this time I got a grade 7. I didn’t even know about this app three days until the exam and it has helped A LOT. Please actually trust me and use it as I’m sure you too will see developments.

Xander S

iOS user

THE QUIZES AND FLASHCARDS ARE SO USEFUL AND I LOVE THE SCHOOLGPT. IT ALSO IS LITREALLY LIKE CHATGPT BUT SMARTER!! HELPED ME WITH MY MASCARA PROBLEMS TOO!! AS WELL AS MY REAL SUBJECTS ! DUHHH 😍😁😲🤑💗✨🎀😮

Elisha

iOS user

This apps acc the goat. I find revision so boring but this app makes it so easy to organize it all and then you can ask the freeeee ai to test yourself so good and you can easily upload your own stuff. highly recommend as someone taking mocks now

Paul T

iOS user

The app is very easy to use and well designed. I have found everything I was looking for so far and have been able to learn a lot from the presentations! I will definitely use the app for a class assignment! And of course it also helps a lot as an inspiration.

Stefan S

iOS user

This app is really great. There are so many study notes and help [...]. My problem subject is French, for example, and the app has so many options for help. Thanks to this app, I have improved my French. I would recommend it to anyone.

Samantha Klich

Android user

Wow, I am really amazed. I just tried the app because I've seen it advertised many times and was absolutely stunned. This app is THE HELP you want for school and above all, it offers so many things, such as workouts and fact sheets, which have been VERY helpful to me personally.

Anna

iOS user

Best app on earth! no words because it’s too good

Thomas R

iOS user

Just amazing. Let's me revise 10x better, this app is a quick 10/10. I highly recommend it to anyone. I can watch and search for notes. I can save them in the subject folder. I can revise it any time when I come back. If you haven't tried this app, you're really missing out.

Basil

Android user

This app has made me feel so much more confident in my exam prep, not only through boosting my own self confidence through the features that allow you to connect with others and feel less alone, but also through the way the app itself is centred around making you feel better. It is easy to navigate, fun to use, and helpful to anyone struggling in absolutely any way.

David K

iOS user

The app's just great! All I have to do is enter the topic in the search bar and I get the response real fast. I don't have to watch 10 YouTube videos to understand something, so I'm saving my time. Highly recommended!

Sudenaz Ocak

Android user

In school I was really bad at maths but thanks to the app, I am doing better now. I am so grateful that you made the app.

Greenlight Bonnie

Android user

very reliable app to help and grow your ideas of Maths, English and other related topics in your works. please use this app if your struggling in areas, this app is key for that. wish I'd of done a review before. and it's also free so don't worry about that.

Rohan U

Android user

I know a lot of apps use fake accounts to boost their reviews but this app deserves it all. Originally I was getting 4 in my English exams and this time I got a grade 7. I didn’t even know about this app three days until the exam and it has helped A LOT. Please actually trust me and use it as I’m sure you too will see developments.

Xander S

iOS user

THE QUIZES AND FLASHCARDS ARE SO USEFUL AND I LOVE THE SCHOOLGPT. IT ALSO IS LITREALLY LIKE CHATGPT BUT SMARTER!! HELPED ME WITH MY MASCARA PROBLEMS TOO!! AS WELL AS MY REAL SUBJECTS ! DUHHH 😍😁😲🤑💗✨🎀😮

Elisha

iOS user

This apps acc the goat. I find revision so boring but this app makes it so easy to organize it all and then you can ask the freeeee ai to test yourself so good and you can easily upload your own stuff. highly recommend as someone taking mocks now

Paul T

iOS user