DSC Chem SAC 1 part a

Last updated almost 6 years ago

39 questions

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DSC Chem SAC 1 part a

Last updated almost 6 years ago

39 questions

Unit 2 SAC 1 part a

This SAC is made up of 15 multiple choice questions and 6 short answer questions.

Please answer all questions in the spaces provided. Please submit your working out at the end of the SAC. (There is a section for working out submission). 
Please make sure your working out is neat, clear and you write which question you are answering next to your working out.

1

2

When KCl and AgNO3 are mixed a precipitate will form.

Write a balanced equation for the reaction using the solubility table provided to predict the precipitate.

Show the states of all chemicals.

(ex. C2H6(g) + 3O2(g) = 2C(s) + 3H2O(g)) Use an equal sign to represent the arrow and don't worry about subscript and superscript

2

When barium nitrate and sodium sulfate are mixed a precipitate will form.

Write a balanced equation for the reaction using the solubility table provided to predict the precipitate.

Show the states of all chemicals.

(ex. C2H6(g) + 3O2(g) = 2C(s) + 3H2O(g)) Use an equal sign to represent the arrow and don't worry about subscript and superscript

2

When sodium iodide and lead (II) nitrate are mixed a precipitate will form.

Write a balanced equation for the reaction using the solubility table provided to predict the precipitate.

Show the states of all chemicals.

(ex. C2H6(g) + 3O2(g) = 2C(s) + 3H2O(g)) Use an equal sign to represent the arrow and don't worry about subscript and superscript

1

Write the net ionic reaction for the KCl and AgNO3 reaction from above

1

Write the net ionic reaction for the barium nitrate and sodium sulfate reaction from above

3

What will be the values of ∆H for
2Al(s) + 3/2 O2(g) → Al2O3(s)

1

3

b. Calculate the amount of energy that will be released from the reaction of 1.00 kg of aluminium.
(*Write you answer below and upload your working out at the end)

3

c. Calculate the amount of energy that will be released from the reaction of 1 kg of oxygen.
(*Write you answer below and upload your working out at the end)

3

Ammonium sulfate, an important fertilizer, can be prepared by the reaction of ammonia with sulfuric acid according to the following balanced equation:

2NH3 (g) + H2SO4(aq) → (NH4)2SO4 (aq)

Calculate the volume of NH3(in litres) needed at 20°C and 25.0atm to react with 150kg of H2SO4.
(*Write you answer below and upload your working out at the end)

Consider the following solubility curves and answer the questions that follow.

0.5

At what temperature is the solubility of CuSO4 • 5H2O 30g/100g?
*Units not needed

0.5

At what temperature is the solubility of CuSO4 • 5H2O 40g/100g?
*Units not needed

1

At what temperature will 60g of KNO3 dissolve in 50g of water?
*Units not needed

0.5

What is the solubility of NaCl at 35°C

0.5

What is the solubility of NaNO3 at 35°C

3

Distinguish between the terms 'unsaturated', 'saturated' and 'supersaturated'.

Propane undergoes complete combustion as follows:
C3H8 (g) + 5O2 (g) → 3CO2 (g) + 4H2O (g)
All volumes are measured at 120°C and 102kPa. 
When 80mL of propane and 500mL of oxygen are reacted:

3

a. One of the gases does not react completely. Which gas is it and how much is unreacted?

2

b. What volumes of carbon dioxide and water are produced in the reaction?

A group of students was conducting an experiment to determine the molar heat of combustion of ethanol. 
They set up the equipment as shown in the diagram below.
They used 200 mL (= 200 g) of water. 
The mass of the spirit burner and ethanol at the beginning of the experiment was 82.5 g and at the conclusion the mass of the spirit burner and remaining ethanol was 81.2 g. 
The maximum temperature rise of the water was found to be 26°C.

3

a. Calculate the students’ experimental value for the molar heat of combustion of ethanol.
(The specific heat of water is 4.18 J K-1 g-1.)
(*Write you answer below and upload your working out at the end)

2

b. When the students consulted their textbook they found the accepted value for the heat of combustion of ethanol to be 1360 kJ/mol, which was different from their experimental value.
Suggest reasons for the difference between the accepted and experimental values.

1

c. Suggest one change which could be made to the experiment to improve the accuracy of the results.

0

Please upload your working out below

Unit 2 SAC 1 part a

This SAC is made up of 15 multiple choice questions and 6 short answer questions.

Please answer all questions in the spaces provided. Please submit your working out at the end of the SAC. (There is a section for working out submission). 
Please make sure your working out is neat, clear and you write which question you are answering next to your working out.

Consider the following equation for the formation of hydrogen chloride gas.

H2(g) + Cl2(g) → 2HCl(g) ΔH = −184 kJ mol−1

When 2 moles of hydrogen gas react completely with 2 moles of chlorine gas:

184 kJ of energy is released

368 kJ of energy is absorbed

368 kJ of energy is released

184 kJ of energy is absorbed

The amount of energy required to raise 150 g of water by 40 °C is:

150 kJ

25 J

150 J

25 kJ

1650 mm Hg is equivalent to how many kPa?

12 379 kPa

219 982 kPa

190 kPa

220 kPa

The mass of 14.2 L of O2(g) measured at SLC is closest to:

9.2 g

10.1 g

18.3 g

20.3 g

Butane gas burns completely in air according to the equation:

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

If 20 mL of butane reacts with 200 mL of oxygen at the same temperature and pressure, the
total volume of gases present at the end of the reaction would be:

250 mL

180 mL

100mL

80 mL

Which of the following terms best describes a substance that dissolves when added to water?

A solvent

A solute

Saturated

Insoluble

Under certain conditions, hydrogen sulfide will burn in oxygen according to the equation:

2H2S(g) + O2(g) → 2S(s) + 2H2O(g)

If all measurements were made at the same temperature and pressure, the volume of water vapour, in mL, produced if 100 mL hydrogen sulfide reacted with 25.0 mL oxygen would be:

100 mL

50.0 mL

25.0 mL

12.5 mL

Which of the following compounds would appear as a precipitate in solution?

ammonium sulfate

ammonium hydroxide

barium sulfate

barium nitrate

Consider the following equation:

aC6H14(g) + bO2(g) → cH2O(g) + dCO(g)

The coefficients that balance the equation are represented by a, b, c and d. These are, respectively:

1, 13, 7, 6

1, 19, 7, 6

2, 19, 14, 12

2, 13, 14, 12

Given
equation 1: 2H2O2(l) → 2H2O(l) + O2(g) ΔH1 = –200 kJ mol–1
equation 2: 2H2(g) + O2(g) → 2H2O(l) ΔH2 = –600 kJ mol–1

ΔH for the reaction H2(g) + O2(g) → H2O2(l) would be:

+200 kJ mol–1

+400 kJ mol–1

–400 kJ mol–1

–200 kJ mol–1

Which of the following is an example of a precipitation reaction?

HCl(aq) + LiOH(aq) → LiCl(aq) + H2O(l)

LiOH(s) → Li+(aq)  + OH-(aq)

NH3(l) + H2O(l) → NH4+(aq) + OH-(aq)

MgSO4(aq) + Ba(NO3)2(aq) → Mg(NO3)2(aq) + BaSO4(s)

Choose the correct statement about the solubility of oxygen gas in water.

The solubility of oxygen gas increases with increased temperature and increased pressure

The solubility of oxygen gas increases with decreased temperature and decreased pressure

The solubility of oxygen gas increases with decreased temperature and increased pressure

The solubility of oxygen gas increases with increased temperature and decreased pressure

The solubility curve for the solution of KNO3 shows that potassium nitrate has a solubility in water of 37 g / 100 g at 20 °C and 110 g / 100 g at 60 °C.

What mass of KNO3 crystals will form if a saturated solution of KNO3 made up in 200g water at 60 °C is cooled to 20 °C?

146 g

73 g

None

37 g

200 g of water and 200 g of ethanol are poured into identical beakers. Both are initially at the same temperature. Each beaker is heated by the addition of 5000 J of heat energy.

Given that the specific heat capacities are:
Ethanol = 2.4 J g–1°C–1
Water = 4.2 J g–1°C–1

You would expect that, after heating, the temperature of the ethanol would be:

higher than that of water, because the specific heat capacity of ethanol is lower than that of water.

the same as that of water because the amount of heat added was the same.

lower than that of water because the hydrogen bonds in ethanol are not as strong as those in water

lower than that of water, because the specific heat capacity of ethanol is lower than that of water.

Select the alternative that represents a balanced equation for incomplete combustion of a fuel.
a.
b.
c. C2H6(g)+ 5O2(g) → 2CO(g) + 3H2O(g)
d.

C2H6(g) + 3O2(g) → 2C(s) + 3H2O(g)

C2H6(g) + 5O2(g) → 2CO(g) + 3H2O(g)

2C2H6(g) + 7O2(g) → 4CO2(g) + 6H2O(g)

2C2H6(g) + 5O2(g) → 4CO(g) + 6H2O(g)

Chemists use solubility tables to decide if an ionic substance is likely to be soluble or not. The table below is a typical example.

Use the infromation above to label each of the following as soluble, slightly insoluble, or insoluble.

AgCl
(NH4)2SO4
CaSO4
NaNO3

Soluble
Slightly Insoluble
Insoluble

When KCl and AgNO3 are mixed a precipitate will form.

Write a balanced equation for the reaction using the solubility table provided to predict the precipitate.

Show the states of all chemicals.

(ex. C2H6(g) + 3O2(g) = 2C(s) + 3H2O(g)) Use an equal sign to represent the arrow and don't worry about subscript and superscript

When barium nitrate and sodium sulfate are mixed a precipitate will form.

Write a balanced equation for the reaction using the solubility table provided to predict the precipitate.

Show the states of all chemicals.

(ex. C2H6(g) + 3O2(g) = 2C(s) + 3H2O(g)) Use an equal sign to represent the arrow and don't worry about subscript and superscript

When sodium iodide and lead (II) nitrate are mixed a precipitate will form.

Write a balanced equation for the reaction using the solubility table provided to predict the precipitate.

Show the states of all chemicals.

(ex. C2H6(g) + 3O2(g) = 2C(s) + 3H2O(g)) Use an equal sign to represent the arrow and don't worry about subscript and superscript

Write the net ionic reaction for the KCl and AgNO3 reaction from above

Write the net ionic reaction for the barium nitrate and sodium sulfate reaction from above

3

What will be the values of ∆H for
2Al(s) + 3/2 O2(g) → Al2O3(s)

1

What will be the values of ∆H for
2Al2O3(s) → 4Al(s) + 3O2(g)

1

What will be the values of ∆H for
Al2O3(s) → 2Al(s) + 3/2 O2(g)

b. Calculate the amount of energy that will be released from the reaction of 1.00 kg of aluminium.
(*Write you answer below and upload your working out at the end)

c. Calculate the amount of energy that will be released from the reaction of 1 kg of oxygen.
(*Write you answer below and upload your working out at the end)

Ammonium sulfate, an important fertilizer, can be prepared by the reaction of ammonia with sulfuric acid according to the following balanced equation:

2NH3 (g) + H2SO4(aq) → (NH4)2SO4 (aq)

Calculate the volume of NH3(in litres) needed at 20°C and 25.0atm to react with 150kg of H2SO4.
(*Write you answer below and upload your working out at the end)

Consider the following solubility curves and answer the questions that follow.

At what temperature is the solubility of CuSO4 • 5H2O 30g/100g?
*Units not needed

At what temperature is the solubility of CuSO4 • 5H2O 40g/100g?
*Units not needed

At what temperature will 60g of KNO3 dissolve in 50g of water?
*Units not needed

What is the solubility of NaCl at 35°C

What is the solubility of NaNO3 at 35°C

Distinguish between the terms 'unsaturated', 'saturated' and 'supersaturated'.

Propane undergoes complete combustion as follows:
C3H8 (g) + 5O2 (g) → 3CO2 (g) + 4H2O (g)
All volumes are measured at 120°C and 102kPa. 
When 80mL of propane and 500mL of oxygen are reacted:

a. One of the gases does not react completely. Which gas is it and how much is unreacted?

b. What volumes of carbon dioxide and water are produced in the reaction?

A group of students was conducting an experiment to determine the molar heat of combustion of ethanol. 
They set up the equipment as shown in the diagram below.
They used 200 mL (= 200 g) of water. 
The mass of the spirit burner and ethanol at the beginning of the experiment was 82.5 g and at the conclusion the mass of the spirit burner and remaining ethanol was 81.2 g. 
The maximum temperature rise of the water was found to be 26°C.

a. Calculate the students’ experimental value for the molar heat of combustion of ethanol.
(The specific heat of water is 4.18 J K-1 g-1.)
(*Write you answer below and upload your working out at the end)

b. When the students consulted their textbook they found the accepted value for the heat of combustion of ethanol to be 1360 kJ/mol, which was different from their experimental value.
Suggest reasons for the difference between the accepted and experimental values.

c. Suggest one change which could be made to the experiment to improve the accuracy of the results.

Please upload your working out below

Consider the following equation for the formation of hydrogen chloride gas.

H2(g) + Cl2(g) → 2HCl(g)  ΔH = −184 kJ mol−1

When 2 moles of hydrogen gas react completely with 2 moles of chlorine gas:

184 kJ of energy is released

368 kJ of energy is absorbed

368 kJ of energy is released

184 kJ of energy is absorbed

The amount of energy required to raise 150 g of water by 40 °C is:

150 kJ

25 J

150 J

25 kJ

1650 mm Hg is equivalent to how many kPa?

12 379 kPa

219 982 kPa

190 kPa

220 kPa

The mass of 14.2 L of O2(g) measured at SLC is closest to:

9.2 g

10.1 g

18.3 g

20.3 g

Butane gas burns completely in air according to the equation:

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

If 20 mL of butane reacts with 200 mL of oxygen at the same temperature and pressure, the
total volume of gases present at the end of the reaction would be:

250 mL

180 mL

100mL

80 mL

Which of the following terms best describes a substance that dissolves when added to water?

A solvent

A solute

Saturated

Insoluble

Under certain conditions, hydrogen sulfide will burn in oxygen according to the equation:

2H2S(g) + O2(g) → 2S(s) + 2H2O(g)

If all measurements were made at the same temperature and pressure, the volume of water vapour, in mL, produced if 100 mL hydrogen sulfide reacted with 25.0 mL oxygen would be:

100 mL

50.0 mL

25.0 mL

12.5 mL

Which of the following compounds would appear as a precipitate in solution?

ammonium sulfate

ammonium hydroxide

barium sulfate

barium nitrate

Consider the following equation:

aC6H14(g) + bO2(g) → cH2O(g) + dCO(g)

The coefficients that balance the equation are represented by a, b, c and d. These are, respectively:

1, 13, 7, 6

1, 19, 7, 6

2, 19, 14, 12

2, 13, 14, 12

Given
equation 1:  2H2O2(l) → 2H2O(l) + O2(g)            ΔH1 = –200 kJ mol–1
equation 2:  2H2(g) + O2(g) → 2H2O(l)               ΔH2 = –600 kJ mol–1

ΔH for the reaction  H2(g) + O2(g) → H2O2(l) would be:

+200 kJ mol–1

+400 kJ mol–1

–400 kJ mol–1

–200 kJ mol–1

Which of the following is an example of a precipitation reaction?

HCl(aq) + LiOH(aq) → LiCl(aq) + H2O(l)

LiOH(s) → Li+(aq)  + OH-(aq)

NH3(l) + H2O(l) → NH4+(aq) + OH-(aq)

MgSO4(aq) + Ba(NO3)2(aq) → Mg(NO3)2(aq) + BaSO4(s)

Choose the correct statement about the solubility of oxygen gas in water.

The solubility of oxygen gas increases with increased temperature and increased pressure

The solubility of oxygen gas increases with decreased temperature and decreased pressure

The solubility of oxygen gas increases with decreased temperature and increased pressure

The solubility of oxygen gas increases with increased temperature and decreased pressure

The solubility curve for the solution of KNO3 shows that potassium nitrate has a solubility in water of 37 g / 100 g at 20 °C and 110 g / 100 g at 60 °C. 

What mass of KNO3 crystals will form if a saturated solution of KNO3 made up in 200g water at 60 °C is cooled to 20 °C?

146 g

73 g

None

37 g

200 g of water and 200 g of ethanol are poured into identical beakers. Both are initially at the same temperature. Each beaker is heated by the addition of 5000 J of heat energy. 

Given that the specific heat capacities are:
Ethanol =  2.4 J g–1°C–1 
Water = 4.2 J g–1°C–1

You would expect that, after heating, the temperature of the ethanol would be:

higher than that of water, because the specific heat capacity of ethanol is lower than that of water.

the same as that of water because the amount of heat added was the same.

lower than that of water because the hydrogen bonds in ethanol are not as strong as those in water

lower than that of water, because the specific heat capacity of ethanol is lower than that of water.

Select the alternative that represents a balanced equation for incomplete combustion of a fuel.
a. 
b.
c. C2H6(g)+ 5O2(g) → 2CO(g) + 3H2O(g)
d. 

C2H6(g) + 3O2(g) → 2C(s) + 3H2O(g)

C2H6(g) + 5O2(g) → 2CO(g) + 3H2O(g)

2C2H6(g) + 7O2(g) → 4CO2(g) + 6H2O(g)

2C2H6(g) + 5O2(g) → 4CO(g) + 6H2O(g)

Chemists use solubility tables to decide if an ionic substance is likely to be soluble or not. The table below is a typical example.

Use the infromation above to label each of the following as soluble, slightly insoluble, or insoluble.

AgCl

(NH4)2SO4

CaSO4

NaNO3

Soluble

Slightly Insoluble

Insoluble

DSC Chem SAC 1 part a

DSC Chem SAC 1 part a

Write the net ionic reaction for the KCl and AgNO3 reaction from above

Write the net ionic reaction for the barium nitrate and sodium sulfate reaction from above

What will be the values of ∆H for 2Al(s) + 3/2 O2(g) → Al2O3(s)

b. Calculate the amount of energy that will be released from the reaction of 1.00 kg of aluminium.(*Write you answer below and upload your working out at the end)

c. Calculate the amount of energy that will be released from the reaction of 1 kg of oxygen.(*Write you answer below and upload your working out at the end)

At what temperature is the solubility of CuSO4 • 5H2O 30g/100g?*Units not needed

At what temperature is the solubility of CuSO4 • 5H2O 40g/100g?*Units not needed

At what temperature will 60g of KNO3 dissolve in 50g of water?*Units not needed

What is the solubility of NaCl at 35°C

What is the solubility of NaNO3 at 35°C

Distinguish between the terms 'unsaturated', 'saturated' and 'supersaturated'.

a. One of the gases does not react completely. Which gas is it and how much is unreacted?

b. What volumes of carbon dioxide and water are produced in the reaction?

a. Calculate the students’ experimental value for the molar heat of combustion of ethanol. (The specific heat of water is 4.18 J K-1 g-1.)(*Write you answer below and upload your working out at the end)

b. When the students consulted their textbook they found the accepted value for the heat of combustion of ethanol to be 1360 kJ/mol, which was different from their experimental value. Suggest reasons for the difference between the accepted and experimental values.

c. Suggest one change which could be made to the experiment to improve the accuracy of the results.

Please upload your working out below

Consider the following equation for the formation of hydrogen chloride gas.H2(g) + Cl2(g) → 2HCl(g) ΔH = −184 kJ mol−1When 2 moles of hydrogen gas react completely with 2 moles of chlorine gas:

The amount of energy required to raise 150 g of water by 40 °C is:

1650 mm Hg is equivalent to how many kPa?

The mass of 14.2 L of O2(g) measured at SLC is closest to:

Butane gas burns completely in air according to the equation:2C4H10(g) + 13O2(g) → 8CO2(g) + 10H2O(g)If 20 mL of butane reacts with 200 mL of oxygen at the same temperature and pressure, thetotal volume of gases present at the end of the reaction would be:

Which of the following terms best describes a substance that dissolves when added to water?

Which of the following compounds would appear as a precipitate in solution?

Consider the following equation:aC6H14(g) + bO2(g) → cH2O(g) + dCO(g)The coefficients that balance the equation are represented by a, b, c and d. These are, respectively:

Givenequation 1: 2H2O2(l) → 2H2O(l) + O2(g) ΔH1 = –200 kJ mol–1equation 2: 2H2(g) + O2(g) → 2H2O(l) ΔH2 = –600 kJ mol–1ΔH for the reaction H2(g) + O2(g) → H2O2(l) would be:

Which of the following is an example of a precipitation reaction?

Choose the correct statement about the solubility of oxygen gas in water.

The solubility curve for the solution of KNO3 shows that potassium nitrate has a solubility in water of 37 g / 100 g at 20 °C and 110 g / 100 g at 60 °C. What mass of KNO3 crystals will form if a saturated solution of KNO3 made up in 200g water at 60 °C is cooled to 20 °C?

Select the alternative that represents a balanced equation for incomplete combustion of a fuel.a. b.c. C2H6(g)+ 5O2(g) → 2CO(g) + 3H2O(g)d.

Chemists use solubility tables to decide if an ionic substance is likely to be soluble or not. The table below is a typical example.Use the infromation above to label each of the following as soluble, slightly insoluble, or insoluble.

Write the net ionic reaction for the KCl and AgNO3 reaction from above

Write the net ionic reaction for the barium nitrate and sodium sulfate reaction from above

What will be the values of ∆H for 2Al(s) + 3/2 O2(g) → Al2O3(s)

What will be the values of ∆H for2Al2O3(s) → 4Al(s) + 3O2(g)

What will be the values of ∆H forAl2O3(s) → 2Al(s) + 3/2 O2(g)

b. Calculate the amount of energy that will be released from the reaction of 1.00 kg of aluminium.(*Write you answer below and upload your working out at the end)

c. Calculate the amount of energy that will be released from the reaction of 1 kg of oxygen.(*Write you answer below and upload your working out at the end)

At what temperature is the solubility of CuSO4 • 5H2O 30g/100g?*Units not needed

At what temperature is the solubility of CuSO4 • 5H2O 40g/100g?*Units not needed

At what temperature will 60g of KNO3 dissolve in 50g of water?*Units not needed

What is the solubility of NaCl at 35°C

What is the solubility of NaNO3 at 35°C

Distinguish between the terms 'unsaturated', 'saturated' and 'supersaturated'.

a. One of the gases does not react completely. Which gas is it and how much is unreacted?

b. What volumes of carbon dioxide and water are produced in the reaction?

a. Calculate the students’ experimental value for the molar heat of combustion of ethanol. (The specific heat of water is 4.18 J K-1 g-1.)(*Write you answer below and upload your working out at the end)

b. When the students consulted their textbook they found the accepted value for the heat of combustion of ethanol to be 1360 kJ/mol, which was different from their experimental value. Suggest reasons for the difference between the accepted and experimental values.

c. Suggest one change which could be made to the experiment to improve the accuracy of the results.

Please upload your working out below

What will be the values of ∆H for2Al2O3(s) → 4Al(s) + 3O2(g)

What will be the values of ∆H forAl2O3(s) → 2Al(s) + 3/2 O2(g)

What will be the values of ∆H for
2Al(s) + 3/2 O2(g) → Al2O3(s)

b. Calculate the amount of energy that will be released from the reaction of 1.00 kg of aluminium.
(*Write you answer below and upload your working out at the end)

c. Calculate the amount of energy that will be released from the reaction of 1 kg of oxygen.
(*Write you answer below and upload your working out at the end)

At what temperature is the solubility of CuSO4 • 5H2O 30g/100g?
*Units not needed

At what temperature is the solubility of CuSO4 • 5H2O 40g/100g?
*Units not needed

At what temperature will 60g of KNO3 dissolve in 50g of water?
*Units not needed

a. Calculate the students’ experimental value for the molar heat of combustion of ethanol.
(The specific heat of water is 4.18 J K-1 g-1.)
(*Write you answer below and upload your working out at the end)

b. When the students consulted their textbook they found the accepted value for the heat of combustion of ethanol to be 1360 kJ/mol, which was different from their experimental value.
Suggest reasons for the difference between the accepted and experimental values.

Consider the following equation for the formation of hydrogen chloride gas.

H2(g) + Cl2(g) → 2HCl(g) ΔH = −184 kJ mol−1

When 2 moles of hydrogen gas react completely with 2 moles of chlorine gas:

Butane gas burns completely in air according to the equation:

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

If 20 mL of butane reacts with 200 mL of oxygen at the same temperature and pressure, the
total volume of gases present at the end of the reaction would be:

Consider the following equation:

aC6H14(g) + bO2(g) → cH2O(g) + dCO(g)

The coefficients that balance the equation are represented by a, b, c and d. These are, respectively:

Given
equation 1: 2H2O2(l) → 2H2O(l) + O2(g) ΔH1 = –200 kJ mol–1
equation 2: 2H2(g) + O2(g) → 2H2O(l) ΔH2 = –600 kJ mol–1

ΔH for the reaction H2(g) + O2(g) → H2O2(l) would be:

The solubility curve for the solution of KNO3 shows that potassium nitrate has a solubility in water of 37 g / 100 g at 20 °C and 110 g / 100 g at 60 °C.

What mass of KNO3 crystals will form if a saturated solution of KNO3 made up in 200g water at 60 °C is cooled to 20 °C?

Select the alternative that represents a balanced equation for incomplete combustion of a fuel.
a.
b.
c. C2H6(g)+ 5O2(g) → 2CO(g) + 3H2O(g)
d.

Chemists use solubility tables to decide if an ionic substance is likely to be soluble or not. The table below is a typical example.

Use the infromation above to label each of the following as soluble, slightly insoluble, or insoluble.

What will be the values of ∆H for
2Al(s) + 3/2 O2(g) → Al2O3(s)

What will be the values of ∆H for
2Al2O3(s) → 4Al(s) + 3O2(g)

What will be the values of ∆H for
Al2O3(s) → 2Al(s) + 3/2 O2(g)

b. Calculate the amount of energy that will be released from the reaction of 1.00 kg of aluminium.
(*Write you answer below and upload your working out at the end)

c. Calculate the amount of energy that will be released from the reaction of 1 kg of oxygen.
(*Write you answer below and upload your working out at the end)

At what temperature is the solubility of CuSO4 • 5H2O 30g/100g?
*Units not needed

At what temperature is the solubility of CuSO4 • 5H2O 40g/100g?
*Units not needed

At what temperature will 60g of KNO3 dissolve in 50g of water?
*Units not needed

a. Calculate the students’ experimental value for the molar heat of combustion of ethanol.
(The specific heat of water is 4.18 J K-1 g-1.)
(*Write you answer below and upload your working out at the end)

b. When the students consulted their textbook they found the accepted value for the heat of combustion of ethanol to be 1360 kJ/mol, which was different from their experimental value.
Suggest reasons for the difference between the accepted and experimental values.

What will be the values of ∆H for
2Al2O3(s) → 4Al(s) + 3O2(g)

What will be the values of ∆H for
Al2O3(s) → 2Al(s) + 3/2 O2(g)