Why it is essential to keep the temperature constant when measuring the progress of the reaction?

Draw a different set of apparatus that could be used to follow the course of reaction between calcium carbonate and hydrochloric acid.

What do you mean by the activation energy?

How does a catalyst work? Select the correct answer from the options below.

Use the collision theory to explain how increasing the surface area of a solid reactant increases the rate of reaction.

Dilute hydrochloric acid reacts with marble chips (calcium carbonate) giving off carbon dioxide gas. Which solution of acid will have the fastest initial rate of reaction

A. $50 {\mathrm{cm}}^3$ of $0.5 \mathrm{mol} {\mathrm{dm}}^3$

B. $10 {\mathrm{cm}}^3$ of $1.0 \mathrm{mol} {\mathrm{dm}}^3$

C. $25 {\mathrm{cm}}^3$of $0.5 \mathrm{mol} {\mathrm{dm}}^3$

Dilute hydrochloric acid reacts with marble chips (calcium carbonate) giving off carbon dioxide gas. Which solution of acid will have the fastest initial rate of reaction

A. $50 {\mathrm{cm}}^3$ of $0.5 \mathrm{mol} {\mathrm{dm}}^3$

B. $10 {\mathrm{cm}}^3$ of $1.0 \mathrm{mol} {\mathrm{dm}}^3$

C. $25 {\mathrm{cm}}^3$of $0.5 \mathrm{mol} {\mathrm{dm}}^3$

Why would B have the fastest initial rate of the reaction?

Which one of these explanations about the effect of increasing the concentration of the reactants on the rate of reaction is completely correct?

What is boltzmann distribution?