Chemical Reactions

State what is meant by the term equilibrium.

Include ideas about rate of reaction and the concentrations of the reactant and products in your answer.

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Predict what happens to the position of equilibrium when the temperature is increased and the pressure remains constant.

Explain your answer.

prediction = ______
explanation = ______

Predict what happens to the position of equilibrium when the pressure is increased and the temperature remains constant.

Explain your answer.

prediction = ______
explanation = ______

Predict what happens to the rate of the backward reaction when the temperature is increased and the pressure remains constant.

Explain your answer.

prediction = ______
explanation = ______

Predict what happens to the rate of the backward reaction when the pressure is increased and the temperature remains constant.

Explain your answer.

prediction = ______
explanation = ______

Explain why the reversible reaction must be in a closed system for an equilibrium mixture to be formed.

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Predict what happens to the position of equilibrium when the temperature is decreased and the pressure remains constant.

Explain your answer.

prediction = ______
explanation = ______

Predict what happens to the position of equilibrium when the pressure is decreased and the temperature remains constant.

Explain your answer.

prediction = ______
explanation = ______

Predict what happens to the rate of the backward reaction when the temperature is decreased and the pressure remains constant.

Explain your answer.

prediction = ______
explanation = ______

Predict what happens to the rate of the backward reaction when the pressure is increased and the temperature remains constant.

Explain your answer.

prediction = ______
explanation = ______

Use the information from the graph to calculate the average speed of reaction in the first two minutes.

Explain why the reaction stopped after 6 minutes.

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On the axes above, sketch a line to show the expected results for the catalysed reaction.

Explain how a catalyst changes the speed of reaction.

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Explain, using ideas about colliding particles, what happens to the speed of this reaction when larger particles of zinc are used.

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Explain, using ideas about colliding particles, what happens to the speed of this reaction when the temperature of the reaction mixture is increased.

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State two conditions for this reaction.

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Describe how, and explain why, the percentage yield changes with temperature.

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Suggest why the reaction is carried out at $300\ ^\circ\text{C}$ and not at $200\ ^\circ\text{C}$.

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Describe how, and explain why, the position of equilibrium changes when the pressure is increased.

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Predict and explain the effect of decreasing the pressure on the position of this equilibrium. The temperature remains constant.

Predict and explain the effect of increasing the concentration of chlorine on the position of this equilibrium.

Describe how the composition of this equilibrium mixture changes with temperature.

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Explain what this tells you about the energy change in this reaction.

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How is the position of equilibrium affected by the presence of a catalyst?

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The rate of this reaction increases with increase in temperature.
Explain why.

the rate of reaction,

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the position of equilibrium.

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the rate of reaction,

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the position of equilibrium.

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The hydration of ethene uses an acid catalyst.

Explain how a catalyst can increase the rate of reaction.

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Describe what is observed during this reaction.

Use the equation to explain that oxidation takes place in this reaction.

Use the equation to explain that reduction takes place in this reaction.

Compounds containing ions of transition elements are often used as catalysts.

Name a catalyst that is the compound of a transition element and state the reaction it catalyses.

name = ______
reaction = ______

Catalysts increase the rate of reaction by providing an alternative reaction pathway with a lower activation energy.

Explain why catalysts are used in industry.

State how long it takes from the start of the experiment to collect $18\,\text{cm}^3$ of hydrogen gas.

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The experiment is repeated at $30\,^\circ\text{C}$.

All other conditions are the same.

Draw a line on the grid to show how the volume of hydrogen gas produced changes with time when the reaction is done at $30\,^\circ\text{C}$.

Describe and explain, using ideas about collisions between particles, how the rate of the reaction changes when the temperature of the reaction mixture is increased.

All other conditions are the same.

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Describe and explain, using ideas about collisions between particles, how the rate of the reaction changes when larger pieces of iron are used.

All other conditions are the same.

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Concentrated sulfuric acid is an oxidising agent.

Describe a test for oxidising agents.

test = ______
observations = ______

The graph shows the volume of hydrogen gas produced at $20^\circ\text{C}$ as the reaction proceeds. The magnesium is in excess.

The experiment is repeated using a lower concentration of hydrochloric acid.

The volume of acid used and all other conditions are the same.

Draw a line on the grid to show how the volume of hydrogen gas produced changes with time when the reaction is done with a lower concentration of hydrochloric acid.

Describe and explain, using ideas about collisions between particles, how the rate of the reaction changes when magnesium powder is used instead of magnesium ribbon.

All other conditions are the same.

Describe and explain, using ideas about collisions between particles, how the rate of the reaction changes when the temperature of the reaction mixture is decreased.

All other conditions are the same.

Magnesium is a good reducing agent.

Describe a test for reducing agents.

test = ______
observations = ______