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What is the rate of a reaction if the value of k is 3 and A and B are each 2 M Rate kA2B?
The rate of the reaction is determined by the rate law, which is typically expressed as Rate = k[A]^m[B]^n, where m and n are the orders of the reactants. If k = 3, A = 2 M, and B = 2 M, and the reaction is kA^2B, then the rate would be 3 x (2)^2 x (2) = 24 M/s.
What is the rate of a reaction if the value of k is 3 and A and B are each 2M?
If the rate law for the reaction is given by rate = k[A]^m[B]^n, where m and n are the orders of the reactants A and B, respectively, then the rate of the reaction would be calculated as rate = k[A][B]. Plugging in the values given (k = 3, A = 2M, B = 2M), the rate of the reaction would be 3*(2)*(2) = 12 M/s.
What is the rate of a reaction if the value of k is 0.01 A is 2 M and B is 3 M Rate kA3B2?
The rate of the reaction is calculated using the rate equation: rate = k[A]^3[B]^2. Given k = 0.01, [A] = 2 M, and [B] = 3 M, the rate can be determined by substituting these values into the rate equation and solving for the rate.
What is the overall reaction order for this rate law rate equals kA2BC?
The overall reaction order for k[A]^2[B][C] would be 4 Because [A] has a rate order of 2 [B] has a rate order of 1 [C] has a rate order of 1 And when you add them together... 2 + 1 + 1 You obtain four
What is the rate reaction if the value of k is 0.01 a is 2 m and b is 3 m rate m a 3 b 2?
.72 (mol/L)/s
What is the rate of a reaction if the value of k is 3 and A and B are each 2 M?
24 (mol/L)s
What is the rate of a reaction if the value of k is 3 and A and B are each 2 M Rate kA2B?
The rate of the reaction is determined by the rate law, which is typically expressed as Rate = k[A]^m[B]^n, where m and n are the orders of the reactants. If k = 3, A = 2 M, and B = 2 M, and the reaction is kA^2B, then the rate would be 3 x (2)^2 x (2) = 24 M/s.
What would happen to the rate of a reaction with rate law ratekNO2H2 if the concentratin of H2 were halved?
Since the reaction is first order with respect to H2, if the concentration of H2 were halved, the rate of the reaction would be halved. This can be seen by entering one for each value in the rate equation, then changing the value of [H2] to 1/2 while keeping the other values the same: The rate changes from 1 to 1/2.
What is the rate of a reaction if the value of k is 3 and A and B are each 2M?
If the rate law for the reaction is given by rate = k[A]^m[B]^n, where m and n are the orders of the reactants A and B, respectively, then the rate of the reaction would be calculated as rate = k[A][B]. Plugging in the values given (k = 3, A = 2M, B = 2M), the rate of the reaction would be 3*(2)*(2) = 12 M/s.
What is the rate of a reaction if the value of k is 0.01 A is 2 M and B is 3 M?
.72
What is the rate of a reaction if the value of k is 0.01 A is 2 M and B is 3 M Rate kA3B2?
The rate of the reaction is calculated using the rate equation: rate = k[A]^3[B]^2. Given k = 0.01, [A] = 2 M, and [B] = 3 M, the rate can be determined by substituting these values into the rate equation and solving for the rate.
What is the overall reaction order for this rate law rate equals kA2BC?
The overall reaction order for k[A]^2[B][C] would be 4 Because [A] has a rate order of 2 [B] has a rate order of 1 [C] has a rate order of 1 And when you add them together... 2 + 1 + 1 You obtain four
What is the rate reaction if the value of k is 0.01 a is 2 m and b is 3 m rate m a 3 b 2?
.72 (mol/L)/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?
0.4 (mol/L)/s
What is the rate constant of a reaction if rate 0.2 (molL)s A and B are each 3 M m 1 and n 2?
7.4 10-3
What would happen to the rate of a reaction with rate law rate k NO 2 H2 if the concentration of H2 were halved?
Halving the concentration of H2 will decrease the rate of the reaction, assuming it is a first-order reaction with respect to H2. Since the rate law is rate = k[NO]^2[H2], cutting the concentration of H2 in half will decrease the rate of the reaction by a factor of 0.5.
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.
