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Reactivity 1. What drives chemical reactions? - IB Questionbank | RevisionDojo

Practice Reactivity 1. What drives chemical reactions? with authentic IB Chemistry exam questions for both SL and HL students. This question bank mirrors Paper 1A, 1B, 2 structure, covering key topics like atomic structure, chemical reactions, and organic chemistry. Get instant solutions, detailed explanations, and build exam confidence with questions in the style of IB examiners.

Paper

Level

Question 1

SL & HLPaper 1A

What is the primary chemical process involved when a fuel is used to release energy?

Question 2

SL & HLPaper 1A

Which of the following fuel sources is considered carbon neutral only if replanted or recycled properly?

Question 3

HLPaper 1A

Which of the following physical states has the highest entropy at a given temperature?

Question 4

HLPaper 1A

A reaction has $\Delta H^\ominus = +100\,\text{kJ}\,\text{mol}^{-1}$ and $\Delta S^\ominus = +250\,\text{J}\,\text{mol}^{-1}\,\text{K}^{-1}$ .

At what minimum temperature (in K) will the reaction become spontaneous?

Question 5

SLPaper 2

When ethane ( $\text{C}_2\text{H}_6$ ) reacts with chlorine gas under UV light, a substitution reaction occurs. This involves breaking the $\text{Cl}-\text{Cl}$ bond to form free radicals before new bonds are made.

Identify the bond being broken in chlorine gas.

[1]

State whether breaking this bond is endothermic or exothermic and justify your answer.

[2]

Define the term bond enthalpy.

[2]

Suggest why ultraviolet light is needed to start this reaction.

[1]

State the bond formed between the carbon atom and the incoming chlorine atom during the substitution.

[1]

Question 6

HLPaper 1A

Which equation represents the standard enthalpy of atomization of bromine, $\text{Br}_2$ ?

Question 7

HLPaper 2

Melting ice is a spontaneous process at room temperature.

Predict the sign of $\Delta S$ for the melting of ice.

[1]

State one reason for this prediction.

[1]

Explain in terms of particle arrangement why entropy increases during melting.

[2]

Question 8

HLPaper 2

Reaction: $\text{H}_2(\text{g}) + \text{I}_2(\text{g}) \to 2\text{HI}(\text{g})$

$\Delta H^\circ = +26\ \text{kJ mol}^{-1}$

$\Delta S^\circ = +164\ \text{J mol}^{-1}\ \text{K}^{-1}$

Calculate $\Delta G^\circ$ at $298\ \text{K}$ .

[2]

Calculate the temperature where $\Delta G^\circ = 0$ .

[2]

Question 9

SL & HLPaper 1A

Which of the following is a renewable energy source?

Question 10

SLPaper 2

A candle is burned in a closed jar with limited oxygen. Over time, black soot forms on the glass, and the flame goes out.

Define incomplete combustion.

[1]

Write a balanced chemical equation for the incomplete combustion of methane forming carbon monoxide.

[1]

State another possible product of incomplete combustion besides carbon monoxide.

[1]

Suggest why incomplete combustion is dangerous in enclosed spaces.

[2]

Compare the energy released in complete and incomplete combustion of the same fuel.

[1]

Paper

Level

Question 1

SL & HLPaper 1A

What is the primary chemical process involved when a fuel is used to release energy?

Question 2

SL & HLPaper 1A

Which of the following fuel sources is considered carbon neutral only if replanted or recycled properly?

Question 3

HLPaper 1A

Which of the following physical states has the highest entropy at a given temperature?

Question 4

HLPaper 1A

A reaction has $\Delta H^\ominus = +100\,\text{kJ}\,\text{mol}^{-1}$ and $\Delta S^\ominus = +250\,\text{J}\,\text{mol}^{-1}\,\text{K}^{-1}$ .

At what minimum temperature (in K) will the reaction become spontaneous?

Question 5

SLPaper 2

Identify the bond being broken in chlorine gas.

[1]

State whether breaking this bond is endothermic or exothermic and justify your answer.

[2]

Define the term bond enthalpy.

[2]

Suggest why ultraviolet light is needed to start this reaction.

[1]

State the bond formed between the carbon atom and the incoming chlorine atom during the substitution.

[1]

Question 6

HLPaper 1A

Which equation represents the standard enthalpy of atomization of bromine, $\text{Br}_2$ ?

Question 7

HLPaper 2

Melting ice is a spontaneous process at room temperature.

Predict the sign of $\Delta S$ for the melting of ice.

[1]

State one reason for this prediction.

[1]

Explain in terms of particle arrangement why entropy increases during melting.

[2]

Question 8

HLPaper 2

Reaction: $\text{H}_2(\text{g}) + \text{I}_2(\text{g}) \to 2\text{HI}(\text{g})$

$\Delta H^\circ = +26\ \text{kJ mol}^{-1}$

$\Delta S^\circ = +164\ \text{J mol}^{-1}\ \text{K}^{-1}$

Calculate $\Delta G^\circ$ at $298\ \text{K}$ .

[2]

Calculate the temperature where $\Delta G^\circ = 0$ .

[2]

Question 9

SL & HLPaper 1A

Which of the following is a renewable energy source?

Question 10

SLPaper 2

A candle is burned in a closed jar with limited oxygen. Over time, black soot forms on the glass, and the flame goes out.

Define incomplete combustion.

[1]

Write a balanced chemical equation for the incomplete combustion of methane forming carbon monoxide.

[1]

State another possible product of incomplete combustion besides carbon monoxide.

[1]

Suggest why incomplete combustion is dangerous in enclosed spaces.

[2]

Compare the energy released in complete and incomplete combustion of the same fuel.

[1]

Paper

Level

Question 1

SL & HLPaper 1A

What is the primary chemical process involved when a fuel is used to release energy?

Question 2

SL & HLPaper 1A

Which of the following fuel sources is considered carbon neutral only if replanted or recycled properly?

Question 3

HLPaper 1A

Which of the following physical states has the highest entropy at a given temperature?

Question 4

HLPaper 1A

A reaction has $\Delta H^\ominus = +100\,\text{kJ}\,\text{mol}^{-1}$ and $\Delta S^\ominus = +250\,\text{J}\,\text{mol}^{-1}\,\text{K}^{-1}$ .

At what minimum temperature (in K) will the reaction become spontaneous?

Question 5

SLPaper 2

Identify the bond being broken in chlorine gas.

[1]

State whether breaking this bond is endothermic or exothermic and justify your answer.

[2]

Define the term bond enthalpy.

[2]

Suggest why ultraviolet light is needed to start this reaction.

[1]

State the bond formed between the carbon atom and the incoming chlorine atom during the substitution.

[1]

Question 6

HLPaper 1A

Which equation represents the standard enthalpy of atomization of bromine, $\text{Br}_2$ ?

Question 7

HLPaper 2

Melting ice is a spontaneous process at room temperature.

Predict the sign of $\Delta S$ for the melting of ice.

[1]

State one reason for this prediction.

[1]

Explain in terms of particle arrangement why entropy increases during melting.

[2]

Question 8

HLPaper 2

Reaction: $\text{H}_2(\text{g}) + \text{I}_2(\text{g}) \to 2\text{HI}(\text{g})$

$\Delta H^\circ = +26\ \text{kJ mol}^{-1}$

$\Delta S^\circ = +164\ \text{J mol}^{-1}\ \text{K}^{-1}$

Calculate $\Delta G^\circ$ at $298\ \text{K}$ .

[2]

Calculate the temperature where $\Delta G^\circ = 0$ .

[2]

Question 9

SL & HLPaper 1A

Which of the following is a renewable energy source?

Question 10

SLPaper 2

A candle is burned in a closed jar with limited oxygen. Over time, black soot forms on the glass, and the flame goes out.

Define incomplete combustion.

[1]

Write a balanced chemical equation for the incomplete combustion of methane forming carbon monoxide.

[1]

State another possible product of incomplete combustion besides carbon monoxide.

[1]

Suggest why incomplete combustion is dangerous in enclosed spaces.

[2]

Compare the energy released in complete and incomplete combustion of the same fuel.

[1]

Reactivity 1. What drives chemical reactions? Questionbank