Description:
The decomposition of N2O5 in carbon tetrachloride proceeds as follows. 2 N2O5---4 NO2 + O2.
The rate law is first order in N2O5. At 64°C the rate constant is 4.82x10^-3 s-1.
rate = k[N2O5]
Questions:
What is the rate of reaction when [N2O5] = 0.0135 M?
What would the rate be when the concentration of N2O5 is doubled to 0.0270 M?
Please answer in M/s.
The decomposition of N2O5 in carbon tetrachloride proceeds as follows. 2 N2O5---4 NO2 + O2.
The rate law is first order in N2O5. At 64°C the rate constant is 4.82x10^-3 s-1.
rate = k[N2O5]
Questions:
What is the rate of reaction when [N2O5] = 0.0135 M?
What would the rate be when the concentration of N2O5 is doubled to 0.0270 M?
Please answer in M/s.
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the first one is 6.507 x 10^-5 M/s
the second is 1.3014 x 10^-4 M/s
the second is 1.3014 x 10^-4 M/s
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For a Nth-order reaction with respect to A,
Rate = k [A]^N = rate constant * concentration of A
So you have k = 4.82 x 10^-3 s^-1 and [N2O5] = 0.0135, and your answer is (4.82 x 10^-3 s^-1 * 0.0135).
Your units work out since your rate constant's units are in s^-1 and concentration in M, so it's M/s.
Rate = k [A]^N = rate constant * concentration of A
So you have k = 4.82 x 10^-3 s^-1 and [N2O5] = 0.0135, and your answer is (4.82 x 10^-3 s^-1 * 0.0135).
Your units work out since your rate constant's units are in s^-1 and concentration in M, so it's M/s.