The initial rates listed in the following table were determined for the reaction
ID: 562884 • Letter: T
Question
The initial rates listed in the following table were determined for the reaction
2NO(g)+Cl2(g)2NOCl(g)
What is the initial rate of reaction when the initial concentrations of both reactants are 0.61 M? (Hint: You must first determine the rate constant and the rate law.)
Enter the results in scientific notation and exponential format. Examples:
Enter for
7.2E-6 7.2x10-6
3.6E-6 3.6x10-6
Experiment Initial[NO] Initial[Cl2] Initial Rate of Consumption ofCl2 (M/s) 1 0.24 0.10 7.2×106 2 0.12 0.10 3.6×106 3 0.12 0.15 5.4×106Explanation / Answer
see experiment 2 and 1:
[NO] doubles
[Cl2] is constant
rate doubles
so, order of NO is 1
see experiment 2 and 3:
[NO] is constant
[Cl2] becomes 1.5 times
rate becomes 1.5 times
so, order of Cl2 is 1
Rate law is:
rate = k*[NO]*[Cl2]
Put values from 1st row of table in rate law
rate = k*[NO]*[Cl2]
7.2*10^-6 = k*0.24*0.1
k = 3*10^-4 M-1.s-1
Now put this in rate law and the concentration of 0.61 M
rate = k*[NO]*[Cl2]
rate = 3*10^-4*0.61*0.61
rate = 1.1*10^-4 M/s
Answer: 1.1*10^-4 M/s
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