At a given temperature, the elementary reaction A↽−−⇀B, in the forward direction, is first order in A with a rate constant of 0.0270 s−1. The reverse reaction is first order in B and the rate constant is 0.0540 s−1. What is the value of the equilibrium constant for the reaction A↽−−⇀B at this temperature? K = ?  What is the value of the equilibrium constant for the reaction B↽−−⇀A at this temperature? K = ?

Given the following rate and concentration data, determine the rate law for the reaction A + B ---> products [A]0 (M) [B]0 (M) initial rate (M/s) 0.10 0.10 4.22 X 10^-6 0.20 0.10 8.44 X 10^-6 0.20 0.40 3.38 X 10^-6 the rate constant k= rate=

Consider this reaction:                        A    +    B    →    C    +    D Expt. [A] (M) [B] (M) Initial Rate (M/s) 1 0.100 0.100 0.152 2 0.100 0.200 0.152 3 0.200 0.200 0.305   What is the overall reaction order for this reaction?

5. The reaction A →→ B + C is known to be first order in A. Below are data showing the concentration of A as a function of reaction time. Time, h 0 1 2 4 8 10 12 [A]. M 1.50 x 10-¹ 1.27 x 10-1 1.07 x 10-1 7.66 x 10-² 3.91 x 10-² 2.80 x 10-2 2.00 x 10-2 (a) What is the average rate of reaction between 1 and 4 h? Report the units as well as the numbers. (b) Plot the data above, showing the concentration of A as a function of the time. From your graph, determine the instantaneous rate of reaction at 8 h. Report the units as well as the numbers. (c) Plot In [A] versus time. Estimate the rate constant for this first-order reaction from your graph. Report the units as well as the numbers.

The rate constant for the reaction is 0.420 M-! ·s- at 200 °C. A → products If the initial concentration of A is 0.00620 M, what will be the concentration after 245 s? [A] = M

ii

Consider a reaction which is 2nd order in regent A. How does the instantaneous rate of the reaction change. When the concentration of A has dropped to 1/2 of its initial value ?

1 of 25 At a given temperature, the elementary reaction A B, in the forward direction, is first order in A with a rate constant of 0.0490 s-. The reverse reaction is first order in B and the rate constant is 0.0960 s-, What is the value of the equilibrium constant for the reaction A B at this temperature? K = What is the value of the equilibrium constant for the reaction B A at this temperature? K = %3D | privacy policy | contact us help terms of use about us careers prime W SapiA II

The rate constant for the second order reaction 2 NO2  2 NO + O2 is 0.31 M-1s-1.  If a 4.33 M sample of NO2reacts for 31.7 seconds, what concentration of NO2 will remain? Report your answer to two decimal places.

At a given temperature, the elementary reaction A = B, in the forward direction, is first order in A with a rate constant of 0.0470 s-1. The reverse reaction is first order in B and the rate constant is 0.0610 s-1. What is the value of the equilibrium constant for the reaction A = B at this temperature? K = What is the value of the equilibrium constant for the reaction B = A at this temperature? K =