# Rate Of Reaction - Effect Of Concentration

4 Questions | Total Attempts: 67

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A quiz to assess your understanding.

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Questions and Answers
• 1.
Why does rate of reaction increase when concentration of reactant increases?
• A.

There are more particles.

• B.

The volume is larger.

• C.

The particles have more energy

• D.

There are more particles per unit volume.

• 2.
Graphs X and Y represent the results of 2 experiments demonstrating the catalytic decomposition of hydrogen peroxide. Assuming that all other conditions are kept constant, which one of the following is a correct explanation of the different results?
• A.

50 cm3 of 1.0 mol/dm3 hydrogen peroxide were used in experiment X while 25 cm3 of 2.0 mol/dm3 of hydrogen peroxide were used in experiment Y

• B.

1.0 g of catalyst was used in experiment X while 0.50 g of catalyst was used in experiment Y.

• C.

Experiment X was carried out at 60 deg celsius while experiment Y was carried out at 30 deg celsius.

• D.

50 cm3 of 1.0 mol/dm3 hydrogen peroxide was used in experiment X while 12.5 cm3 of 2.0 mol/dm3 were used in experiment Y.

• 3.
Magnesium reacts with hydrochloric acid. Which solution would give the fastest initial rate of reaction given that the same volume of each acid is used?
• A.

1 mol/dm3 of HCl

• B.

2 mol/dm3 of citric acid, a tribasic acid

• C.

1 mol/dm3 of H2SO4

• D.

0.5 mol/dm3 of H2SO4

• 4.
In the graph, curve (I) was obtained when 1 g of granulated zinc reacted with an excess of hydrochloric acid at 30 °C. Which of the following changes to this reaction would give curve (ii) ?
• A.

Using 0.5 g of granulated zinc

• B.

Using 1 g of finely powdered zinc

• C.

Warming the acid to 40 °C.

• D.

Adding water to dilute the acid