Conclusion: B is not in the rate law expression.

Different reactions can happen at different rates. Reactions that happen slowly have a low rate of reaction. Reactions that happen quickly have a high rate of reaction. For example, the chemical weathering of rocks is a very slow reaction: it has a low rate of reaction. Explosions are very fast reactions: they have a high rate of reaction.

Problem #1: Rate data were obtained for following reaction:A + 2B --- C + 2D

Problem #7: Determine the proper form of the rate law for:CH3CHO(g) ---> CH4(g) + CO(g)

1) Note experiments 2 and 3.

There are two ways to measure the rate of a reaction:

If the activation energy is high only a small
amount of particles will have enough energy to react so the reaction rate would
be very small, however, if the activation energy is very low the number of
particles with that amount of energy will be high so the reaction rate would be

A chemistry quiz on reaction rates

In this piece of science coursework I will be experimenting how the rate of reaction between Sodium thiosulphate and hydrochloric acid is affected by the concentration of Sodium thiosulphate.


This article presents an assignment in which students are to research and report on a chemical reaction whose increased or decreased rate is of practical importance. Specifically, students are asked to represent the reaction they have chosen with an acceptable chemical equation, identify a factor that influences its rate and explain how and why it does so, and describe the relevance of the reaction occurring at a slower or faster rate under this condition. The assignment is designed to develop and assess a number of valuable skills and understandings, including the ability to write effectively.

AP Chem-035 The Rate of Reactions — bozemanscience

Therefore we had no problem with too
much gas.

This is the apparatus we used to measure the amount of H2 that was produced in
the reactions.

Rates of Reaction - GCSE Science - Marked by …

The rate of reaction depends on the rate of successful collisions between reactant particles. The more successful collisions there are, the faster the rate of reaction.


For example, if 24cm3 of hydrogen gas is produced in two minutes, the mean rate of reaction = 24 ÷ 2 = 12cm3 hydrogen / min.