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They are experimentally determined exponents.

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Determine the rate of a reaction that follows the rate law rate kAmBn where k 0.2 A 3 M B 3 M m 1 n 2?

5.4 (apex)


What is the rate of a reaction that follows the rate law rate kAmBn where k 0.2 A3 M B3 M m1 n2?

The rate of the reaction can be calculated using the rate law equation rate = k[A]^m[B]^n. Plugging in the given values k = 0.2, m = 1, n = 2, [A] = 3 M, and [B] = 3 M into the equation gives rate = 0.2 * (3)^1 * (3)^2 = 16.2 M/s.


What is k Rate kAmBn?

In the context of chemistry, "k Rate kAmBn" refers to the rate constant (k) of a reaction involving reactants A and B, where "m" and "n" represent the stoichiometric coefficients of these reactants in the rate law. The rate of the reaction can be expressed as proportional to the concentrations of A and B raised to their respective powers, leading to the equation: rate = k [A]^m [B]^n. This relationship helps in understanding how changes in concentration affect the speed of the reaction.


Determine the rate of a reaction that follows the rate law rate kAmBn where k 1.5 A 1 M B 3 M m 2 n 1?

4.5 (mol/L)/s


What is the rate of a reaction that follows the rate law rate kAmBn if k 0.02 A and B are each 3 M m 2 and n 3?

The rate of the reaction can be calculated using the rate law rate = k[A]^m[B]^n. Plugging in the given values: rate = 0.02*(3)^3*(3)^3 = 0.022727 = 14.58 M/s.


Which equation is an expression of the rate law?

Rate = k[A]m[B]n


What are m and n in the rate law equation?

They are experimentally determined exponents


What equation is an expression of the rate of law?

r=[A]m[B]n APPLEX


How can one effectively write a rate law for a chemical reaction?

To write a rate law for a chemical reaction, one must determine the order of the reaction with respect to each reactant by conducting experiments and analyzing the rate of reaction at different concentrations. The rate law is then expressed as rate kAmBn, where k is the rate constant, A and B are the concentrations of the reactants, and m and n are the orders of the reaction with respect to each reactant.


What equation shows how rate depends on concentrations of reactions?

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.


What units must the rate constant have based on the rate law, and can you provide an example of how to calculate it?

The rate constant must have units that make the rate equation balanced. For example, if the rate law is rate kA2B, the rate constant k must have units of M-2 s-1. To calculate the rate constant, you can use experimental data and the rate law equation to solve for k.


Which equation would be used to calculate the rate constant from inital concentrations?

To calculate the rate constant (k) from initial concentrations, you would typically use the rate law equation for the reaction, which is expressed as ( \text{Rate} = k[A]^m[B]^n ), where ( [A] ) and ( [B] ) are the initial concentrations of the reactants, and ( m ) and ( n ) are their respective reaction orders. By measuring the initial rate of the reaction and substituting the initial concentrations into the rate law, you can rearrange the equation to solve for the rate constant ( k ).