IB Chemistry SL 2.2.3 Factors Affecting Rate Questions

Use real SL experiments and curves to predict and explain how reaction conditions change rate while controlling other variables.

Exam points

Predict how concentration, pressure, temperature, surface area or a catalyst changes reaction rate and the product-versus-time curve.
Explain pressure, concentration and surface-area effects through collision frequency, and temperature effects through kinetic energy and the fraction above activation energy.
Distinguish a catalyst effect on rate from a change in the final amount of product or equilibrium position, keeping other conditions controlled.

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Study 2.2.3—Factors affecting rate conceptsOpen the corresponding Concept lesson for explanations, examples and exam connections.

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0.100 g of magnesium ribbon is added to $50.0 \mathrm{~cm}^{3}$ of $1.00 \mathrm{moldm}^{-3}$ sulfuric acid to produce hydrogen gas and magnesium sulfate.

\mathrm{Mg}(\mathrm{~s})+\mathrm{H}_{2} \mathrm{SO}_{4}(\mathrm{aq}) \rightarrow \mathrm{H}_{2}(\mathrm{~g})+\mathrm{MgSO}_{4}(\mathrm{aq})

The graph shows the volume of hydrogen produced against time under these experimental conditions.

Figure for Question IB Chemistry SL 2.2.3 Factors Affecting Rate Questions question 1 — IB Chemistry SL

Sketch two curves, labelled I and II, to show how the volume of hydrogen produced (under the same temperature and pressure) changes with time when:

I. using the same mass of magnesium powder instead of a piece of magnesium ribbon;
II. 0.100 g of magnesium ribbon is added to $50 \mathrm{~cm}^{3}$ of $0.500 \mathrm{moldm}^{-3}$ sulfuric acid.

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IB Chemistry SL 2.2.3 Factors Affecting Rate Questions question 1