Search results
order with respect to each reactant reflects the molecularity of the process (how many molecules are involved). For example, Unimolecular decomposition A → B ν = k [A] Bimolecular reaction A + B → P ν = k [A][B] A + A → P ν = k [A][A] = k [A]2
- 322KB
- 31
In a reaction between E and F, the reaction was found experimentally to be second order overall. Which of the following mechanisms is consistent with this. Explain your answer.
- 67KB
- 2
The overall rate of a reaction is determined by the rate of the slowest in its mechanism, called the rate-determining step. Unimolecular elementary reactions have first-order rate laws, while bimolecular elementary reactions have second-order rate laws.
Explain what is meant by the term "rate of reaction". 2. The initial rates of the reaction 2A + B 2C + D at various concentrations of A and B are given below: a) What is the order of reaction with respect to A and B? b) What is the overall order of reaction? c) What is the rate constant?
- 12KB
- 2
1. Write the rate equation in each of the following cases. For each example, state the overall order of the reaction. a) The reaction A + 2B = C + D, where the rate of reaction isn't affected by the concentration of A, but is proportional to the square of the concentration of B.
- 56KB
- 1
Selected examples are given to highlight these reactions in the context of complex molecule synthesis. An effort has been made to provide students with references that encourage further reading on a given topic.
People also ask
What is Order of a reaction with respect to a reactant?
What is an example of zero order reaction?
Do bimolecular elementary reactions have first-order rate laws?
What is an example of first order reaction?
What is the rate constant for pseudo first order reaction?
Do all elementary steps in a valid reaction mechanism combine?
• define the average and instantaneous rate of a reaction; • express the rate of a reaction in terms of change in concentration of either of the reactants or products with time; • distinguish between elementary and complex reactions; • differentiate between the molecularity and order of a reaction; • define rate constant;
