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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.
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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.
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 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 ).
Which is necessary to determine the rate of a reaction using the rate of law?
To determine the rate of a reaction using the rate law, you need the rate constant (k), the concentrations of the reactants, and the reaction order with respect to each reactant. The rate law expresses the relationship between the rate of the reaction and the concentrations of the reactants raised to their respective powers, which correspond to the reaction orders. Experimental data is required to establish these parameters accurately.
What is the rate of a reaction if the value of k is 0.1 a is 1m and b is 2m?
To find the rate of the reaction, you can use the rate law equation. If the reaction is of the form ( \text{Rate} = k [A]^m [B]^n ), and assuming that ( A ) and ( B ) have a reaction order of 1 (i.e., ( m = 1 ) and ( n = 1 )), the rate would be calculated as follows: [ \text{Rate} = 0.1 \times (1, \text{m}) \times (2, \text{m}) = 0.2, \text{mol/L/s} ] Thus, the rate of the reaction is 0.2 mol/L/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)
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.
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 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.
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 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 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 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 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 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 zero order reaction rate law and how does it determine the rate of a chemical reaction?
The zero order reaction rate law states that the rate of a chemical reaction is independent of the concentration of the reactants. This means that the rate of the reaction remains constant over time. The rate of the reaction is determined solely by the rate constant, which is specific to each reaction. This rate law is expressed as: Rate k, where k is the rate constant.
