10 questions🇬🇧English
⏱️ Rates of Reaction – GCSE
Chemistry · GCSE — collision theory, factors affecting rate, catalysts and reading rate graphs
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Questions
According to collision theory, what must happen for reactant particles to react?
They must be dissolved in water
They must collide at any speed
They must collide with enough energy
They must be heated to boiling point
20s
What is meant by the activation energy of a reaction?
Energy released when the products form
Total energy stored in the reactants
Minimum energy colliding particles need to react
Energy needed to melt the reactants
20s
How does a catalyst increase the rate of a reaction?
It increases the concentration of reactants
It gives the particles more kinetic energy
It provides a pathway with lower activation energy
It raises the activation energy of the reaction
20s
Why does raising the temperature increase the rate of a reaction?
Heating creates more reactant particles
Particles collide more often and with more energy
The activation energy of the reaction decreases
Particles collide more often but with less energy
30s
Powdered marble reacts faster with hydrochloric acid than large marble chips of equal mass. Why?
Larger surface area gives more frequent collisions
The powder contains more calcium carbonate
The powder particles have more kinetic energy
The powder has a lower activation energy
30s
Increasing the pressure of reacting gases speeds up the reaction. What is the main reason?
More particles in the same volume, so more collisions
The gas particles become larger
Each gas particle moves faster at higher pressure
The activation energy becomes lower
30s
In the disappearing cross practical, sodium thiosulfate reacts with hydrochloric acid. What makes the mixture go cloudy?
A precipitate of sodium chloride
Bubbles of hydrogen gas
A precipitate of sulfur
Bubbles of carbon dioxide
30s
As gas escapes from a reaction, the mass falls. Mass is measured in grams and time in seconds. Which is the correct unit for rate?
g/s
g/cm³
g × s
s/g
20s
A reaction produces 48 cm³ of gas in the first 16 seconds. What is the mean rate of reaction over this time?
768 cm³/s
3 cm³/s
0.33 cm³/s
32 cm³/s
30s
On a graph of gas volume against time, how do you find the rate of reaction at one particular time?
Find the area under the curve up to that time
Divide the total volume by the total time
Read off the volume of gas at that time
Draw a tangent there and find its gradient
30s