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C3 Quantitative Chemistry

Last updated about 1 month ago
190 questions
4.3.1.1 Conservation of mass and balanced chemical equations
2

Balance the following equation, use (1, 2, 3, 4) to input the balanced equation.

2

Balance the following equation, use (1, 2, 3, 4) to input the balanced equation.

2

Balance the following equation, use (1, 2, 3, 4) to input the balanced equation.

2

Balance the following equation, use (1, 2, 3, 4) to input the balanced equation.

2

Balance the following equation, use (1, 2, 3, 4) to input the balanced equation.

1

What are the coefficients for the reaction N2 + O2 → NO2, in the order in which the reaction is written?

1

What are the coefficients for the reaction CH4 + O2 → CO2 + H2O, in the order in which the reaction is written?

1

What are the coefficients for the reaction H2O → H2 + O2, in the order in which the reaction is written?

1

How many carbon atoms are in C3H7O2?

1

How many hydrogen atoms are in C3H7O2?

1

How many oxygen atoms are in C3H7O2?

1
1
3

Balance the Equation(use the format of 2, 4, 1)

___Al + _____Br2 → ____AlBr3

3

Balance the Equation(use the format of 2, 4, 1)

____SrO → ____Sr + ____O2

3

Balance the Equation(use the format of 2, 4, 1)

____HF→ ____H2 + ____F2

3

Balance the Equation(use the format of 2, 4, 1)

____Rb + ___N2 → ___Rb3N

4

Balance the Equation(use the format of 2, 4, 1, 3)

____KI + ____F2 → ____KF + ___I2

1

I take 100g of water and stir in 50g of sugar. What is the mass of the sugar water?

1

I take 77g of Lead Nitrate and 20g of Potassium Iodide. The solution turns bright yellow. What is its mass?

1

If 10 grams of substance A reacts with 15 grams of substance B, what should be the resulting mass according to the Law of Conservation of Mass?

1

5 grams of iron reacts with 10 grams of oxygen to form rust. What is the total mass of the rust?

1

Carbon (12 g) reacts with Oxygen (16 g) to form carbon dioxide. What is the mass of the carbon dioxide?

1

20 grams of ice melts into water. According to the Law of Conservation of Mass, what is the mass of the water?

1

I heat some 100g of iron in air and form iron oxide, following this equation

2Fe + O2 --> 2FeO

I weighed my new iron oxide and found it weighed 105g. Why?

1

I react Calcium carbonate and hydrochloric acid together like this

HCl(aq) + CaCO3(s) --> CO2(g) + H2O(l) + CaCl2(aq)

I start with 200g of reactants, but when I weigh my reactants they don't weight 200g! Why is that?

A pupil heated 1.24g of copper carbonate strongly.
The chemical reaction, which took place, is represented
by the equation:

CuCO3(s) --> CuO(s) + CO2(g)

After the solid, which remained, had cooled, he weighed it. He found that its mass was 0.80g
1

Why did the pupil find a decrease in mass in this experiment?

1

He then heated the 0.80g of solid again. When he weighed it after cooling, its mass was still 0.80g. Explain why it had not changed in mass this time.

1

In another experiment, he burnt magnesium ribbon in air. He found that the mass of the powder formed was greater than the original mass of the ribbon. Explain this.

1

Write a balanced equation for the reaction, which takes place when the magnesium burns in oxygen.

1
Carbon monoxide is produced by the incomplete combustion of methane.

Balance the equation for the reaction.

2CH4 + 3O2 → _______ CO + 4H2O
1
This question is about displacement reactions.

Iron is extracted from iron oxide by a displacement reaction with carbon.

 Balance the equation for the reaction.

Fe2O3 + 3C → _______Fe + _______CO
1

The Haber Process is used to produce ammonia from nitrogen and hydrogen.

The equation for the reaction is:

N2  +  3H2  ⇌  2NH3

An ammonia molecule has the formula NH3

How many atoms are there in one molecule of ammonia?

Tick (✔) one box

1

Maria fills a bowl with 200 g of water. She puts the bowl of water in the freezer, and the water freezes. Which will most likely be the mass of the frozen water?

1

If reaction starts with 20g of reactants it should produce...

1

If you put 200 grams of ice into a pitcher with 900 grams of water. Then get distracted and come back later to find that the ice has melted in the water. How many grams of water do you now have in the pitcher?

1

A student mixes 125 grams of sugar, 250 grams of water and 5 grams of flavoring. The solution weighs...

1

24 g of magnesium reacts with 38 g of fluorine to produce _____ g magnesium fluoride

1

In the reaction AB-----> A + B reactant AB has 12g and product B has 5g. How many grams should product A have?

5

This question is worth 5 points. Take some time to create your own infographic of the law of conservation of mass.

Must have:
* "The Law of Conservation of Mass" definition
* a written example of the law of conservation of mass
* a picture or pictures to go with your examples

Here are some helpful examples:
Example 1 link
Example 2 link

Required
1

Indicate whether the chemical equation supports the law of conservation of mass.

Required
1

Indicate whether the chemical equation supports the law of conservation of mass.

Required
1

Indicate whether the chemical equation supports the law of conservation of mass.

Ecosystems have many chemical and physical changes happening all at once, and matter is conserved in each and everyone—no exceptions. Consider a stream flowing through a canyon—how many chemical and physical changes are happening at any given moment? What would happen if matter continuously disappeared during these reactions?

You just finished learning how balancing chemical equations is required to uphold the law of conservation of matter. Now it's time to put your knowledge to the test. Using PhET's Balancing Chemical Equations Simulation.

Directions:

  • Enter the PhET Simulation website or use the interactive embedded below.
  • Start with the Introduction section.
1. Check out the simulation's controls.
2. Answer each pre-lab question.
  • Enter the game section, by clicking "Game" on the simulation's bottom black menu bar.
  1. Test your balancing ability at all three levels. Each level requires you to balance 5 equations. You must score at least 4 stars at each level to earn full credit.
  2. Take a screenshot of your Game Results screen with all three levels for the last question.
  3. Add a screenshot of your Game Results screen with all three levels.
1

What law is being demonstrated by the simulation?

3

Match each substance to its correct coefficient to balance the chemical equation for ammonia.
N2 + H2 --> NH3

Draggable itemCorresponding Item
H2
3
N2
1
NH3
2
2

Which compounds have a coefficent of 2 to separate water?

1

It is possible to balance the provided equations by leaving a substance with a coefficient of 0.

4

Drag each substance to its correct coefficient to balance the chemical equation for methane.

  • O2
  • CO2
  • CH4
  • H2O
  • 1
  • 2
  • 3
1
Carbon monoxide is produced by the incomplete combustion of methane.

Balance the equation for the reaction.

2CH4 + 3O2 → _______ CO + 4H2O
1
This question is about displacement reactions.

Iron is extracted from iron oxide by a displacement reaction with carbon.

 Balance the equation for the reaction.

Fe2O3 + 3C → _______Fe + _______CO
1
Balance the equation below so that it follows the Law of Conservation of Mass?

__________HCl + __________Na --> __________NaCl + __________H2
1
Balance this chemical equation by adding the correct coefficients

4Al+3O₂-----> _______ Al₂O₃
1
Balance the equation below so that it follows the Law of Conservation of Mass?

__________H2+ O2 → __________H2O
2

Balance the following equation, use (1, 2, 3, 4) to input the balanced equation.

2

Balance the following equation, use (1, 2, 3, 4) to input the balanced equation.

2

Balance the following equation, use (1, 2, 3, 4) to input the balanced equation.

2

Balance the following equation, use (1, 2, 3, 4) to input the balanced equation.

2

Balance the following equation, use (1, 2, 3, 4) to input the balanced equation.

1

What are the coefficients for the reaction N2 + O2 → NO2, in the order in which the reaction is written?

1

What are the coefficients for the reaction CH4 + O2 → CO2 + H2O, in the order in which the reaction is written?

1

What are the coefficients for the reaction H2O → H2 + O2, in the order in which the reaction is written?

4.3.1.2 Relative Formula Mass
2

Calculate the molar mass of Li2S. Specifically rounded to the tenth. Work is worth one point.

1

The atomic mass of N is 14, and the atomic mass of H is 1.0. What is the formula mass of NH3?

1

Given the atomic masses O=16, Na=23, find the relative formula mass of Na2O.

1

If the atomic masses are C=12, H=1, and O=16, calculate the relative formula mass of H2O.

1

Given the atomic masses S=32, H=1, O=32, calculate the relative formula mass of H2SO4.

1

Given that F=19, Na=23, calculate the relative formula mass of NaF.

1

Calculate the relative formula mass of F2

1

Calculate the relative formula mass of Fe

1

Calculate the relative formula mass of H2SO4

1

Calculate the relative formula mass of Al2O3

1

Calculate the relative formula mass of Mg(OH)2

1

Calculate the relative formula mass of Al(NO3)3

1

Calculate the relative formula mass of (NH4)2SO4

1

Calculate the relative formula mass of CuCO3

1

Calculate the relative formula mass of AgNO3

1

Calculate the relative formula mass of NH4NO3

1

Calculate the relative formula mass of CuSO4.5H2O

1

Calculate the relative formula mass of magnesium.

1

Calculate the relative formula mass of oxygen.

1

Calculate the relative formula mass of sodium bromide.

1

Calculate the relative formula mass of calcium fluoride.

1

Calculate the relative formula mass of potassium sulfate.

1

Calculate the relative formula mass of chlorine.

1

Calculate the relative formula mass of chromium(III) oxide.

1

Calculate the relative formula mass of sodium.

1

Calculate the relative formula mass of iron(III) sulfate.

4.3.1.3 Mass changes when a reactant or product is a gas
4.3.1.4 Chemical measurements
4.3.2.1 Moles

For the following questions, you'll need to use this formula to work out mass or moles for the following questions.
2

How many moles is 25.1 g H2O given the molar mass of H2O is 18.0 g/mol?

1

What is the mass of 2.75 moles of CaO? CaO=56

1

Calculate the moles of NaCl in 200 g. NaCl=58.5

1

Determine the mass of 7.88 moles of copper

1

Convert 25.0 grams of NaCl into moles. NaCl = 58.5

1

Calculate the mass of epsom salt that would contain 0.085 moles of magnesium sulfate (MgSO4). Mg=12, S=32, O=16

1

How many moles are in 85 g of AgNO3? (round to two decimal places)

1

How many grams are there in 1.3 moles of BaO?

1

The Hope Diamond has a mass of 9.10 grams. Diamonds have a very simple chemical formula, they only contain carbon. How many moles of carbon are in the Hope Diamond?

1

Calculate the number of moles in 220g of CO2

1

Calculate the number of moles in 168g of CO

1

Calculate the number of moles in 234g of NaCl

1

Calculate the number of moles in 26g of LiF

1

Calculate the number of moles in 128g of SO2

4.3.2.2 Amounts of substances in equations
Hello! I'm Miss Bryant - In the AQA Spec, this is called 'Reacting Masses'. Our American friends describe this as 'Stoichiometry'.

But when I teach this, using the method below, I call it 'Down Across and Up', which I think is unique to me.

It is essentially 3 calculations

1) Convert known mass into moles
2) Account for the ratio
2) Use these moles and convert into mass - this is your answer
1

Calculate the mass of aluminium that can be formed from1020 g of aluminium oxide.

2Al2O3 → 4Al + 3O2

1

Calculate the mass of oxygen needed to react 10.0 g of calcium to form calcium oxide.

2Ca + O2 → 2CaO

1

What mass of propane could burn in 48.0 g of oxygen? 1 dp please!

C3H8 + 5O2 → 3CO2 + 4H2O

1

What mass of ammonia can be made from 20.0 g of hydrogen? Please round to a whole number

3H2 + N2 → 2NH3

1

What mass of sodium hydroxide is needed to neutralise 24.5 kg of sulfuric acid? Please include units!

H2SO4 + 2NaOH → Na2SO4 + 2H2O

1

What mass of carbon dioxide is formed when 7.41 g of copper(II) carbonate decomposes on heating? 2 dp please!

CuCO3 → CuO + CO2

1

What mass of carbon monoxide is needed to react with 2.08 kg of iron oxide? Please answer in grams

Fe2O3 + 3CO → 2Fe + 3CO2

1

What mass of chlorine reacts with 20.0 g of iron to form iron(III) chloride?

2Fe + 3Cl2 → 2FeCl3

1

Hydrazine (N2H4) is used as a rocket fuel. It can be made by reacting ammonia with hydrogen peroxide. What mass of ammonia is needed to make 148 g of hydrazine?

2NH3 + H2O2 → N2H4 + 2H2O

4.3.2.3 Using moles to balance equations
1

5.8 g of butane (C4H10) reacts with 20.8 g of oxygen (O2) during complete combustion.

Find the ratio of Butane:Oxygen

1

11.6 g of tungsten oxide (WO3) reacts with 0.30 g of hydrogen (H2) during the extraction of tungsten.

Find the ratio Tungen Oxide: Hydrogen

1

2.56 g of sulfur dioxide (SO2) reacts with 0.64 g of oxygen (O2) to form sulfur trioxide.

Find the ratio of Sulfur Dioxide:Oxygen

1

0.920 g of silver carbonate (Ag2CO3) decomposes to form 0.773 g of silver oxide (Ag2O) and 0.147 g of carbon dioxide (CO2).

Find the ratio of Silver Carbonate : Silver Oxide : Carbon Dioxide

1

10.00 g of octadecane (C18H38) decomposes on heating in a cracking reaction to form 2.28 g of butane (C4H10), 3.31 g of propene (C3H6) and 4.41 g of ethene (C2H4).

Find the ratio of Octadecane:Butane:Propene:Ethene

1

4.00 g of potassium hydrogencarbonate (KHCO3) decomposes on heating to form 2.76 g of potassium carbonate (K2CO3), 0.88 g of carbon dioxide (CO2) and some water (H2O).

Find the ratio of Potassium Hydrogencarbonate:Potassium Carbonate:Carbon Dioxide:Water

4.3.2.4 Limiting reactants
1

How many complete pens can you make?

1

What is the limiting factor?

1

How many pens can you make?

1

What is the limiting factor?

1

How many pens can you make?

1

What is in excess?

1

A + B --> C

How much C can you make if...


3 mol of A and 5 mol of B

1

A + B --> C

How much C can you make if...


8 mol of A and 6 mol of B

1

A + B --> C

How much C can you make if...


0.2 mol of A and 0.15 mol of B

1

P + 2Q --> R

How much R can you make if....

4 mol of P and 6 mol of Q

1

P + 2Q --> R

How much R can you make if....

10 mol of P and 24 mol of Q

1

P + 2Q --> R

How much R can you make if....

0.2 mol of P and 0.5 mol of Q

4.3.2.5 Concentration of solutions
1

Convert 200 cm3 to dm3.

1

Convert 750 cm3 to dm3.

1

Convert 1500 cm3 to dm3.

1

Convert 85 cm3 to dm3.

1

Convert 2.5 dm3 to cm3.

1

What is 3.2 dm3 in cm3?

1

Change 1.7 dm3 to cm3.

1

Transform 4.8 dm3 into cm3.

9

Match the following terms with the correct definition

Draggable itemCorresponding Item
hydration
A homogeneous mixture of solute and solvent
saturated solution
The substance that is dissolved in the solution
solution
The substance, usually water, in which another substance is dissolved
solvent
The amount of solute per unit volume of solution
concentrated solution
A solution of known concentration
dissociation
A solution with a lots of moles of solute per unit volume
standard solution
A solution that has more solute than it can dissolve.
concentration
Process where existing ions of an ionic compound are separated in solution
solute
Achieved when ions are completely dissolved in a solution
Required
1

Convert 10 cm3 to dm3

Required
1

Convert 25 cm3 to dm3

Required
1

Convert 0.064 dm3 to cm3

Required
1

Step 1

Required
1

Step 2

Required
1

Step 3

Required
1

Step 1

Required
1

Step 2

Required
1

Step 3

Required
3

(a) Either use the canvas directly to show your work or complete in your notebook & upload a picture into the canvas.

Required
3

(b) Either use the canvas directly to show your work or complete in your notebook & upload a picture into the canvas.

Required
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(c) Either use the canvas directly to show your work or complete in your notebook & upload a picture into the canvas.

Required
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(a) Either use the canvas directly to show your work or complete in your notebook & upload a picture into the canvas.

Required
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(b) Either use the canvas directly to show your work or complete in your notebook & upload a picture into the canvas.

Required
3

(c) Either use the canvas directly to show your work or complete in your notebook & upload a picture into the canvas.

4.3.3.1 Percentage yield
1

A chemist performs a reaction expected to yield 50g of product but collects only 40g. Determine the percentage yield of the reaction.

1

If an experiment results in 30g of product with a theoretical yield of 60g, what is the percentage yield?

1

A reaction has a theoretical yield of 75g but 25g of product is actually recovered. Calculate the percentage yield of the reaction.

1

A reaction has an actual yield of 20g and a theoretical yield of 80g. What is the percentage yield?

1

In this reaction, the theoretical yield of copper sulfate was 14.5 g. However, only 8.6 g were produced. Calculate the percentage yield.

1

Calculate the percentage yield for each of the following reactions given the actual and theoretical yields.
a Zoe makes 20.5 g of copper chloride.
The maximum possible amount she could have made is 35.6 g.

1

George isolates 5.6 g of a clean, dry precipitate of iron(II) hydroxide.
The maximum possible amount he could have isolated is 15.3 g.

1

The teacher tells Aivija that she could theoretically make 1.26 mol of aspirin.
When she carries out the reaction she finds she has made 0.87 mol.

1

Iron is made by reduction of iron oxide with carbon monoxide.

Fe2O3 + 3CO → 2Fe + 3CO2

a) Calculate the mass of iron that can be formed from 126 g of iron oxide

1

b) 78.5 g of iron was formed in this reaction. Calculate the percentage yield.

1

Chlorine can be made by the electrolysis of sodium chloride solution.

2NaCl + 2H2O → 2NaOH + Cl2 + H2

a) Calculate the mass of chlorine that can be formed from 50.0 g of sodium chloride.

1

b) 25.0 g of chlorine was formed in this reaction. Calculate the percentage yield.

1

Chromium is a useful metal. It is extracted from chromium oxide by reaction with aluminium.

Cr2O3 + 2Al → 2Cr + Al2O3

a) Calculate the mass of chromium that can be formed from 1.25 kg of chromium oxide.

1

b) 756 g of chromium was formed in this reaction. Calculate the percentage yield.

4.3.3.2 Atom economy
1

The reaction between ethene and steam to produce ethanol is represented by the equation: C2H4 + H2O --> C2H5OH

If 98 g of ethene is used, what is the maximum mass of ethanol that can be produced? (Ar values: C = 12.0, H = 1.0, O = 16.0)

1

The reaction between ethene and steam to produce ethanol is represented by the equation: C2H4 + H2O --> C2H5OH

Which statement is true?

1

1. The hydrogen used in the Haber process is produced from natural gas, containing methane. The equation for this stage of the process is: CH4 + 2H2O --> CO2 + 4H2
Calculate the atom economy for the production of hydrogen. (Ar values: C = 12.0, H = 1.0, O = 16.0)

1

Calculate the atom economy to form copper(II) oxide from copper(II) carbonate. CuCO3 → CuO + CO2

1

Calculate the atom economy to form aluminium from aluminium oxide. 2Al2O3 → 4Al + 3O2

1

Calculate the atom economy to form iron from iron oxide. Fe2O3 + 3CO → 2Fe + 3CO2

1

Calculate the atom economy to form aluminium chloride from aluminium in this reaction. 2Al + 3Cl2 → 2AlCl3

1

Calculate the atom economy to form oxygen from hydrogen peroxide. 2H2O2 → 2H2O + O2

1

Hydrogen (H2) has many uses, including as the fuel in many fuel cells. It can be made in several ways. a) Calculate the atom economy to form hydrogen by method 1. CO + H2O → CO2 + H2

1

b) Calculate the atom economy to form hydrogen by method 2. CH4 + 2H2O → CO2 + 4H2

1

When choosing which method to use, one factor to consider is the atom economy. In terms of atom economy, which method is preferable.

1

What, apart from atom economy, be considered when choosing between methods?

4.3.4 Using concentrations of solutions in mol/dm 3
4.3.5 Use of amount of substance in relation to volumes of gases
1

Find the volume of the following gas, at room temperature and pressure (assume answer is in dm3):

4.00 moles of oxygen

1

Find the volume of the following gas, at room temperature and pressure (assume answer is in dm3):

0.250 moles of methane

1

Find the volume of the following gas, at room temperature and pressure (assume answer is in dm3):

15 moles of Argon

1

Find the volume of the following gas, at room temperature and pressure (assume answer is in dm3):

0.220 g of Carbon Dioxide (CO2)

1

Find the number of moles of the following gas, at room temperature and pressure (assume answer is in moles):

48.0 dm3 of Carbon Monoxide

1

Find the number of moles of the following gas, at room temperature and pressure (assume answer is in moles):

1.20 dm3 of Hydrogen

1

Find the number of moles of the following gas, at room temperature and pressure (assume answer is in moles):

360 cm3 of Oxygen

1

Find the volume of oxygen gas that reacts with 10 dm3 of sulfur dioxide gas measured at the same temperature and pressure.

2SO2(g) + O2(g) → 2SO3(g)

1

Find the volume of hydrogen gas that reacts with 200 cm3 of nitrogen gas measured at the same temperature and pressure. Please answer in dm3

N2(g) + 3H2(g) → 2NH3(g)

1

Find the volume of oxygen that reacts with 4.0 dm3 of butane (C4H10) gas measured at same temperature & pressure.

2C4H10(g) + 13O2(g) → 8CO2(g) + 10H2O(l)

1

I want to make some oxygen for my Yr 9, so they can learn the gas test for it. I have 100g of Hydrogen Peroxide.

H2O2 --> H2 + O2

How much Oxygen can I produce?

1

What size of measuring cylinder would I need to invert to catch all the oxygen?