Rate law is:
rate = k*[A]*[B]
Put values from 1st row of table in rate law
rate = k*[A]*[B]
2.65*10^-4 = k*0.0155*0.00211
k = 8.10 M-1.s-1
Answer:
8.10
M-1.s-1
Reaction 2A + B --> 3C is first order in B and zero order in A. The initial concentrations are 0.250M for A and B and 0.000M for C. The rate constant for a certain temperature is 1.30 x 10-3 s-1. Write down the rate law for this reaction in terms of disappearance of the reactant B. Calculate reaction half-life Calculate the molarity of B after 50.0 sec. Calculate the molarity of product C after 50.0 sec. Calculate molarity of...
2A → B + C The above reaction is run and found to follow first order kinetics with a rate constant of 1.30 x 10-3 sec-1. If the initial concentration of A is 1.73 M, what is the concentration after 133 seconds?
If the rate law for the reaction2A + 3B ? productsis first order in A and second order in B, then the rate law is rate = ________________.a. k [A] [B]b. k [A]2 [B]3c. k [A] [B]2d. k [A]2 [B]e. k [A]2 [B]2
Given A + 3B 2C + D This reaction is first order with respect to reactant A and second order with respect to reactant B. If the concentration of A is doubled and the concentration of B is halved, the rate of the reaction would ________ by a factor of _______.
The following reaction is second order in respect to NO and first order in respect to H2. The rate constant was found to be 0.67 M-2· s-1. If the reaction starts with 0.200 M NO and 0.350 M H2, calculate the initial reaction rate. Group of answer choices 0.0094 M/s 0.047 M/s 0.014 M/s 0.0022 M/s
Consider the equation: 2A + B → C The initial rate of reaction is measured at several different concentrations of the reactants with the following results: [A] (M) [B] (M) Initial Rate (M/s) 0.40 0.10 0.026 0.10 0.10 0.026 0.40 0.20 0.103 (blank 1) What is the order with respect to reactant A? (write a number) (blank 2) What is the order with respect to B? (write a number) (blank 3) What is the value of the rate constant. Include...
The reaction: 2A → C is first order. If the initial concentration of A is 1.0M and the rate constant is 5.9 x 10-3s-1 , What is the final concentration of A after 3.0 minutes? A. 0.35 B. 0.98 C. 0.94
You have a reaction: A + B --> C The reaction is first order with respect to A and 2nd order with respect to B. If 0.8904 mol of A is mixed with 0.3749 mol of B to make a 1.000 L solution and the rate of the reaction is 0.873 M/s, what is the rate constant (k)?
The reaction between phenolphthalein and hydroxide ion is first order with respect to the phenolphthalein and zero order with respect to the hydroxide. Calculate the rate constant for this reaction when the instantaneous rate of reaction is 2.5 x 10-5moles per liter per second for a concentration of 0.00250 M for the phenolphthalein. Group of answer choices a. 0.010 M-1 s-1 b. 2.5 x 10-5M/s c. 0.010 s-1 d. 0.010 M-2 s-1 e. cannot be determined from the given information
The reaction 2A B is first order in A with a rate constant of 2.8 x 10-25-2 at 80°C. How long in seconds) will it take for A to decrease from 0.800 M to 0.140 M?