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In the rate law equation ( \text{rate} = k[A]^m[B]^n ), ( m ) and ( n ) represent the reaction orders with respect to the reactants ( A ) and ( B ), respectively. These values indicate how the reaction rate is affected by the concentrations of the reactants: ( m ) shows the sensitivity of the rate to changes in concentration of ( A ), while ( n ) does the same for ( B ). The orders are determined experimentally and can be whole numbers, fractions, or zero, depending on the reaction mechanism.
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What is the rate of a reaction that follows the rate law rate kAmBn if k 02 A and B are each 3 M m 2 and n3?
To determine the rate of the reaction that follows the rate law rate = k[A]^m[B]^n, where k = 3 M^(-2) s^(-1), [A] = 2 M, and [B] = 3 M, we first need to substitute these values into the rate law. Given that m = 2 and n = 3, the rate can be calculated as follows: Rate = k[A]^m[B]^n = 3 M^(-2) s^(-1) * (2 M)^2 * (3 M)^3 = 3 * 4 * 27 = 324 M/s. Thus, the rate of the reaction is 324 M/s.
How does the rate law show how concentration changes affet the rate of reaction?
The rate law expresses the relationship between the rate of a chemical reaction and the concentrations of the reactants. It is typically formulated as Rate = k[A]^m[B]^n, where k is the rate constant, and m and n are the reaction orders for reactants A and B, respectively. The exponents indicate how the rate is affected by changes in concentration; for example, if m = 1, doubling the concentration of A will double the reaction rate, whereas if m = 2, the rate will quadruple. Thus, the rate law quantitatively illustrates how variations in reactant concentrations influence the overall reaction rate.
How can the rate constant be determined fro the rate law?
The rate constant can be determined from the rate law by rearranging the rate equation to isolate the rate constant (k). Typically, the rate law is expressed as ( \text{Rate} = k [A]^m [B]^n ), where ( [A] ) and ( [B] ) are the concentrations of reactants and ( m ) and ( n ) are their respective reaction orders. By measuring the reaction rate at known concentrations of the reactants, you can calculate k using the formula ( k = \frac{\text{Rate}}{[A]^m [B]^n} ). This requires experimental data to provide the necessary values for rate and concentrations.
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 1and n 2?
To find the rate of the reaction, we can use the given rate law: ( \text{rate} = k[A]^m[B]^n ). Substituting the values, we have ( k = 0.02 , \text{M}^{-1}\text{s}^{-1} ), ( [A] = 3 , \text{M} ), and ( [B] = 3 , \text{M} ) with ( m = 1 ) and ( n = 2 ). Thus, the rate is calculated as: [ \text{rate} = 0.02 \times (3)^1 \times (3)^2 = 0.02 \times 3 \times 9 = 0.54 , \text{M/s} ] Therefore, the rate of the reaction is 0.54 M/s.
What is the rate of a reaction that follows the rate law rate kAmBn if k is 02 A and B are each 3 M m 2 and n3?
To find the rate of the reaction following the rate law rate = k[A]^m[B]^n, we substitute the values given: ( k = 0.2 , \text{M}^{-2} , \text{s}^{-1} ), ( [A] = 3 , \text{M} ), and ( [B] = 3 , \text{M} ) with ( m = 2 ) and ( n = 3 ). The rate can be calculated as follows: [ \text{Rate} = 0.2 \cdot (3)^2 \cdot (3)^3 = 0.2 \cdot 9 \cdot 27 = 48.6 , \text{M/s}. ] Thus, the rate of the reaction is 48.6 M/s.
What is the rate of a reaction that follows the rate law rate kAmBn if k 02 A and B are each 3 M m 2 and n3?
To determine the rate of the reaction that follows the rate law rate = k[A]^m[B]^n, where k = 3 M^(-2) s^(-1), [A] = 2 M, and [B] = 3 M, we first need to substitute these values into the rate law. Given that m = 2 and n = 3, the rate can be calculated as follows: Rate = k[A]^m[B]^n = 3 M^(-2) s^(-1) * (2 M)^2 * (3 M)^3 = 3 * 4 * 27 = 324 M/s. Thus, the rate of the reaction is 324 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 rate kAmBn?
They are experimentally determined exponents.
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.
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 general form of a rate law?
The general form of a rate law is rate = k[A]^m[B]^n, where rate is the reaction rate, k is the rate constant, [A] and [B] are the concentrations of reactants A and B, and m and n are the respective reaction orders for A and B.
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.
How does the rate law show how concentration changes affet the rate of reaction?
The rate law expresses the relationship between the rate of a chemical reaction and the concentrations of the reactants. It is typically formulated as Rate = k[A]^m[B]^n, where k is the rate constant, and m and n are the reaction orders for reactants A and B, respectively. The exponents indicate how the rate is affected by changes in concentration; for example, if m = 1, doubling the concentration of A will double the reaction rate, whereas if m = 2, the rate will quadruple. Thus, the rate law quantitatively illustrates how variations in reactant concentrations influence the overall reaction rate.
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 an expression of the rate law?
r=[A]m[B]n APPLEX
What are m and n in the rate law equation?
They are experimentally determined exponents
How can the rate constant be determined fro the rate law?
The rate constant can be determined from the rate law by rearranging the rate equation to isolate the rate constant (k). Typically, the rate law is expressed as ( \text{Rate} = k [A]^m [B]^n ), where ( [A] ) and ( [B] ) are the concentrations of reactants and ( m ) and ( n ) are their respective reaction orders. By measuring the reaction rate at known concentrations of the reactants, you can calculate k using the formula ( k = \frac{\text{Rate}}{[A]^m [B]^n} ). This requires experimental data to provide the necessary values for rate and concentrations.
