The reaction X + Y --> products was studied using the method of initial rates. T

Question

The reaction X + Y --> products was studied using the method of initial rates. The initial rate of consumption of X was measured in three different experiments. Data are provided below.

Expt [X] o
1(in mol/L) [Y] o
2(in mol/L) Initial Rate
3(in mol L -1 s - 1 )
1= 0.700, 0.600, 1.517
2= 2.10, 0.600, 0.5057
3= 0.700, 1.50, 9.482

What is the value of the rate constant, k? (Use concentrations in mol/L and time in seconds. Enter your answer accurate to three significant figures.)

Hint: First determine the rate law, and then evaluate k.

Explanation / Answer

If you plot -ln[O] vs. t, you expect a straight line, and you get [O]/[O]initial = exp(-kt) one with slope = 100.15. real rate equation is: Rate = k[NO2][O] The slope of 100.15 isn't k, it is actually k[NO2], since the slope came from psuedo-first-order reaction data with excess NO2. So, 100.15 = k[NO2] k = 100.15/(1.0 x 10^13) = 1.0 x 10^-11 M^-1 s^-1

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