Day 1  Day 2  Day 3  Day 4  Day 5  Day 6

Day 1

Question 1

The equations for two reactions are shown.

 Equation 1 C + CO2​​ ​​ xCO

 Equation 2 2C2H6​​ + 7O2​​ ​​ 4CO2​​ + yH2O

Which row shows the value of x, the value of y and the equations that are for redox reactions?

Question 2

Four redox equations are statements about the equations are shown.

Which statements about the equations are correct?

• 1 and 2

• 1 and 3

• 2 and 4

• 3 and 4

Day 2

Question 1

The equations for the reaction of metal M with aqueous zinc sulfate is shown.

M + ZnSO4​​ ​​ MSO4​​ + Zn

Which statement explains why metal M reacts with aqueous zinc sulfate?

• Zinc is less reactive than M because M is able to accept electrons from zinc ions.

• Zins is a more powerful reducing agent than M.

• Zinc is more reactive than M because it can lose electrons more easily than M.

• Zinc ions can remove electrons from M.

Question 2

In which equation is the underlined substance acting as a reducing agent?

• 3CO​​ + Fe2O3​​ ​​ 2F2 + 3CO2

• CO2​​ + C​​ ​​ 2CO

• CuO​​ + H2​​ ​​ Cu + H2O

• CaO​​ + H2O – Ca(OH)2

Day 3

Question 1

Magnesium powder reacts with an excess of dilute hydrochloric acid to produce hydrogen gas.

Which statements about this reaction are correct?

• The smaller the particles of magnesium powder, the more slowly the hydrogen is produced.

• The higher the temperature, the faster the magnesium powder disappears.

• The lower the concentration of dilute hydrochloric acid, the faster the rate of reaction.

• The faster the magnesium powder disappears, the faster the rate of reaction.

• 1 and 2

• 2 and 3

• 2 and 4

• 3 and 4

Question 2

Excess magnesium ribbon is reacted with a fixed volume of hydrochloric acid and the volume of gas given off over time is measured.

The results of two different experiments are shown.

Which statement explains the differences between the results of the two experiments?

• Reactions 1 uses a catalyst.

• The acid used is twice as concentrated in reaction 1.

• The magnesium ribbon is in smaller pieces in reaction 2.

• The temperature is higher in reaction 2.

Day 4

Question 1

A student adds excess zinc to dilute hydrochloric acid at 25​​ oC.

The hydrogen gas produced is collected and measured at room temperature and pressure.

The results are plotted and labelled as curve X on the graph.

The experiment is repeated at 50​​ oC with all other conditions remaining the same.

Which graph shows the results at 50​​ oC?

Question 2

The reaction between two aqueous compounds, X and Y, is slow and exothermic.​​ 

The graph shows hoe the rate of this reaction changes with time.

A student suggests that the rate of reaction decreases with time because:

• The activation energy decreases.

• The speed of the molecules of X and Y decreases.

• The concentration of both X and Y decreases with time.

Which suggestions are correct?

• 1 and 2

• 1 and 3

• 2 only

• 3 only

Day 5

Question 1

Hydrogen reacts with iodine to form hydrogen iodide.

H2​​ + I2​​ ​​ 2HI

Which statements explain why the reaction is faster when the pressure is increased, at constant temperature?

• At higher pressure, the molecules are moving faster.

• At higher pressure, more of the molecules have the required activation energy.

• At higher pressure, the molecules are closer together.

• At higher pressure, the molecules collide more frequently.

• 1 and 2

• 1 and 3

• 2 and 4

• 3 and 4

Question 2

Which row describes the effect on the activation energy and the frequency of particle collisions when the temperature of a chemical reaction is increased?

Day 6

Question 1

Hydrogen peroxide, H2O2, decomposes to form water and oxygen.

2H2O2​​ ​​ 2H2O + O2

Manganese(IV) oxide catalyses the decomposition reaction.

The reaction is investigated in four experiments.

All reactions go to completion and all measurements of gas volumes are at room temperature and pressure.

Which statement is correct?

• Experiment 1 produces less gas than experiment 4, but at the same rate.

• Experiment 2 produces more gas than experiment 4, but at the same rate.

• Experiment 2 and experiment 4 each produce the same volume of gas, but at different rates.

• Experiment 3 and experiment 4 each produce the same volume of gas and at the same rate.

Question 2

Which row describes the effect of increasing concentration and increasing temperature on the collisions between reacting particles?