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What are m and n in the rate law equation rateK(A)m(B)n?
In the rate law equation ( \text{rate} = k[A]^m[B]^n ), ( m ) and ( n ) represent the reaction orders with respect to reactants ( A ) and ( B ), respectively. These values indicate how the rate of the reaction changes in response to changes in the concentrations of the reactants. They are determined experimentally and can be whole numbers or fractions, reflecting the complexity of the reaction mechanism.
What equation is an expression of the rate of law?
r=[A]m[B]n APPLEX
What 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?
To determine the rate of the reaction using the rate law ( \text{rate} = k[A]^m[B]^n ), we can substitute the values given. With ( k = 1.5 , \text{M}^{-2}\text{s}^{-1} ), ( [A] = 1 , \text{M} ), ( [B] = 3 , \text{M} ), ( m = 2 ), and ( n = 1 ), the rate can be calculated as follows: [ \text{rate} = 1.5 \times (1)^2 \times (3)^1 = 1.5 \times 1 \times 3 = 4.5 , \text{M/s} ] Thus, the rate of the reaction is ( 4.5 , \text{M/s} ).
What is the rate of a reaction if the value of k is 0.1 is 1 M and B is 2 M?
To calculate the rate of a reaction, you typically use the rate law equation, which can be expressed as ( \text{Rate} = k[A]^m[B]^n ), where ( k ) is the rate constant, ( [A] ) and ( [B] ) are the concentrations of the reactants, and ( m ) and ( n ) are their respective orders. Assuming a simple first-order reaction with respect to both A and B (i.e., ( m = n = 1 )), the rate would be calculated as ( \text{Rate} = 0.1 \times (1)^1 \times (2)^1 = 0.2 , \text{M/s} ). Thus, the reaction rate is 0.2 M/s.
What is the rate of a reaction if the value of k is 0.1 A is 1 M and B is 2 M Rate kA2B2?
To calculate the rate of the reaction using the rate law ( \text{Rate} = k[A]^m[B]^n ), where ( k = 0.1 ), ( [A] = 1 , \text{M} ), and ( [B] = 2 , \text{M} ), we first need to determine the values of ( m ) and ( n ). Assuming the reaction is second-order in A and second-order in B (i.e., ( m = 2 ) and ( n = 2 )), the rate would be calculated as: [ \text{Rate} = 0.1 \times (1)^2 \times (2)^2 = 0.1 \times 1 \times 4 = 0.4 , \text{M/s}. ] Thus, the rate of the reaction is 0.4 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 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
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 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.
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 are m an n in the rate law eqation rate k(A)(b)?
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.
What is the rate of reaction that follows the rate of law rate k AmB?
The rate of reaction that follows the rate law ( \text{Rate} = k [A]^m [B]^n ) indicates that the reaction rate depends on the concentrations of reactants ( A ) and ( B ), raised to their respective powers ( m ) and ( n ). The constant ( k ) is the rate constant, which is specific to the reaction at a given temperature. The values of ( m ) and ( n ) represent the order of the reaction with respect to each reactant, which can be determined experimentally. Overall, the overall order of the reaction is the sum ( m + n ).
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.
What equation is an expression of the rate of law?
r=[A]m[B]n APPLEX
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)
