What is the unit of constant rate in chemical master equation?
Answers
Explanation:
Using the general form:rate = k [A]^a [B]^bthe units of k have to cancel out the concentration units to make sure that rate is in molarity / second.
- So for first order, where rate = k [A],k is in s^-1; second order
(rate = k [A]^2 or rate = k [A] [B]) k must be in M^-1 s^-1.
Answer:
The rate law or rate equation for a chemical reaction is an equation that links the initial or forward reaction rate with the concentrations or pressures of the reactants and constant parameters (normally rate coefficients and partial reaction orders).[1] For many reactions, the initial rate is given by a power law such as
{\displaystyle v_{0}\;=\;k[\mathrm {A} ]^{x}[\mathrm {B} ]^{y}} {\displaystyle v_{0}\;=\;k[\mathrm {A} ]^{x}[\mathrm {B} ]^{y}}
where [A] and [B] express the concentration of the species A and B, usually in moles per liter (molarity, M). The exponents x and y are the partial orders of reaction for A and B and the overall reaction order is the sum of the exponents. These are often positive integers, but they may also be zero, fractional, or negative. The constant k is the reaction rate constant or rate coefficient of the reaction. Its value may depend on conditions such as temperature, ionic strength, surface area of an adsorbent, or light irradiation. If the reaction goes to completion, the rate equation for the reaction rate {\displaystyle v\;=\;k[\mathrm {A} ]^{x}[\mathrm {B} ]^{y}} {\displaystyle v\;=\;k[\mathrm {A} ]^{x}[\mathrm {B} ]^{y}} applies throughout the course of the reaction.