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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.
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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 K in the right large reaction rate equals K a MB and?
In the expression for the reaction rate, ( K ) represents the rate constant, which is a proportionality factor that quantifies the relationship between the concentration of reactants (in this case, ( a ), ( M ), and ( B )) and the rate of the reaction. The value of ( K ) is dependent on factors such as temperature and the specific reaction mechanism. It reflects the intrinsic properties of the reaction and is essential for predicting how the reaction rate changes with varying concentrations of reactants.
What has the largest value of the constant k?
how does the rate law show how concentration changes after the rate of reaction
Find a formula for Poiseuilles Law given that the rate of flow is proportional to the fourth power of the radius and Use k as the proportionality constant?
Rate of flow varies as R^4 where R is the radius or Rate of flow = (k) x (R^4)
What is formula of rate constant?
The rate constant, often denoted as ( k ), is a proportionality factor in the rate law of a chemical reaction. Its formula depends on the order of the reaction. For a first-order reaction, ( k ) has units of ( s^{-1} ), while for a second-order reaction, it has units of ( M^{-1}s^{-1} ). The general expression for the rate law can be represented as ( \text{Rate} = k[A]^n ), where ( [A] ) is the concentration of the reactant and ( n ) is the reaction order.
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 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.
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 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 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 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 k in the rate law equation?
A rate constant
What is an apparent rate constant?
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.
The concentration of both A and B was doubled the reaction rate also doubled What is the rate law for this reaction?
The rate law for this reaction is rate = k[A][B], where the rate constant k is doubled along with the concentrations of A and B.
How can one determine the rate constant k in a chemical reaction?
The rate constant k in a chemical reaction can be determined by conducting experiments to measure the reaction rate at different concentrations of reactants. By plotting the data and using the rate equation, the rate constant k can be calculated.
