Consider the following reaction: A + B → products. The rate law was found to be rate = k[A][B]^2. A)What is the order with respect to A? B)What is the order with respect to B? C)What is the overall order of the reaction?
- Consider the following reaction: A + B → products. The rate law was found to be rate = k[A][B]^2.
A)What is the order with respect to A?
B)What is the order with respect to B?
C)What is the overall order of the reaction?
D)If the concentration of A is doubled while the concentration of B is kept constant, how will this affect the
E)If the concentration of B is doubled while the concentration of A is kept constant, how will this affect the rate of the reaction? How will this affect the time required for the reaction to reach completion?
F)If the concentration of B is doubled while the concentration of A is halved, how will this affect the rate of the reaction? How will this affect the time required for the reaction to reach completion?
Given rate =k[A][B]^2
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