Useful formulas/constants: 1/[A] = 1/[A]_0 + kt ln ([A]_0/[A]) = kt R = 0.0821 L
ID: 536060 • Letter: U
Question
Useful formulas/constants: 1/[A] = 1/[A]_0 + kt ln ([A]_0/[A]) = kt R = 0.0821 L*atm/mol*K R = 8.314 J/mol*K. The decomposition of hydrogen peroxide, 2 H_2O_2 rightarrow 2H_2O + O_2, was run in a laboratory. The following data was obtained: a) What is the overall order of this reaction? Explain. You must show complete proof of this answer on a separate piece of paper for full credit. b) What is the value of the rate constant? c) What is the final concentration of hydrogen peroxide after 1124 seconds? d) What is the half-life (t_1/2) of hydrogen peroxide? Below is a graph when the ln k vs. 1/T is graphed for the following reaction: N_2O_5 rightarrow 2 NO_2 + 1/2 O_2. What is the value of the rate constant at 300 degree C if it is 2.5*10^-3 s^-1 at 280 degree C?Explanation / Answer
a) For that purpose, we have to calculate the rate at two 2-3 different concentrations
rate = change in concentration/time = 0.185/60 = 0.003 M/s (concentration at 0.882)
If we are taking next two,
rate = 0.169/60 = 0.0028 M/s (concentration at 0.697)
Take the ratio of rates at these = 1.16
and the concentrations is = 1.2
If the ratio of these two is giving a value 1 it is first order and if it is giving a value 4 it is 2nd order
in this case, it is giving a value 0.97 which is close to 1 and the reaction is a first order reaction
b) rate = k [H2O2], we calculated rate is 0.0028 at 0.697 M concentration of H2O2
0.0028 = k 0.697O
k = 0.004 s-1
c) For a first order reaction half life = 0.693/k
= 0.693/0.004 = 173.25 s
As per the policy of Chegg only one question is answered
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