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A relative rate constant the rate at which a reaction will take place. Ex. V = k [A][B] the constant ,k, is a constant value for the rate of the reaction in said equation.
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Here it is in two forms: k = A exp (-Ea/RT) ln k = ln A - Ea/RT The latter is a linearized version. In both cases... k is the rate constant, A is the frequency factor (an experimentally determined quantity related to the probability that a collision will lead to a reaction), Ea is the activation energy, R is the Universal Gas constant (8.31 J/mol K), and T is the temperature in Kelvins.
The rate constant is the reaction rate divided by the concentration terms.
The equation is called the rate law equation. For the reaction aA+bB =>cC+dD the rate law would be rate = k[A]^m[B]^n where k is the rate constant and m and n are the "order" with respect to each reactant. m and n must be determined experimentally and may or may not be the same as the coefficients a and b.
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First order rate constant k is described in V=k[EA] while second order rate constant is given as V=k[E][A]. For reactions that do not have true order, k is the apparent rate constant.
A rate constant
A relative rate constant the rate at which a reaction will take place. Ex. V = k [A][B] the constant ,k, is a constant value for the rate of the reaction in said equation.
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how does the rate law show how concentration changes after the rate of reaction
chemical changes causing leaves to brown in the fall
how does the rate law show how concentration changes after the rate of reaction
k=Rate/[A^m][B^n]
A relative rate constant the rate at which a reaction will take place. Ex. V = k [A][B] the constant ,k, is a constant value for the rate of the reaction in said equation.
K = constant