A certain reaction is second order in N2 and second order in H2 . Use this information to complete the table below. Round each of your answers to 3 significant digits. First row: [N2] is 0.237 M, [H2] is 0.455 M, and the initial rate of reaction is 0.678 M/s. Second row: [N2] is 0.0591 M, [H2] is 0.455 M, find the initial rate of reaction. Third row: [N2] is 0.985 M, [H2] 0.109 M, calculate initial rate of reaction.
To determine the rate constant (k) for a second-order reaction, we can use the rate equation:
rate = k[N2]^2[H2]^2
First, let's use the given information from the first row to calculate the rate constant (k):
0.678 M/s = k*(0.237 M)^2*(0.455 M)^2
Solving for k:
k = (0.678 M/s) / (0.237 M)^2*(0.455 M)^2
k ≈ 16.073 M^-3/s
Now, let's use the calculated rate constant (k) to find the initial rate of reaction in the second and third rows.
Second row:
[N2] = 0.0591 M
[H2] = 0.455 M
rate = k*[N2]^2*[H2]^2
rate = (16.073 M^-3/s)*(0.0591 M)^2*(0.455 M)^2
rate ≈ 0.033 M/s
Third row:
[N2] = 0.985 M
[H2] = 0.109 M
rate = k*[N2]^2*[H2]^2
rate = (16.073 M^-3/s)*(0.985 M)^2*(0.109 M)^2
rate ≈ 0.485 M/s
So, the initial rates of reaction in the second and third rows are approximately 0.033 M/s and 0.485 M/s, respectively.