Question

The initial concentration of N2O5 in the following first oder reaction N2O5 - - - > 2NO2v+1/2O2 was 1.24*
10^-2 mol/L at 318 k. the concentration of N2O5 after 60 min. was 0.20*10^-2 mol/L calculate the rate constant of the reaction at 318k.​

Answer 1

here is your answer mate

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Answer 2

Answer: The rate constant for the given reaction is $0.3041min^{-1}$

Explanation:

We are given that the reaction is first order kinetics. The equation used to calculate the rate constant for first order kinetics is:

$k=\frac{2.303}{t}\log\frac{a}{a-x}$

where,

k = rate constant of the reaction  = ?

t = time taken for decay process = 60 min

a = initial amount of the reactant  = $1.24\times 10^{-2}mol/L$

a - x = amount left after decay process  = $0.2\times 10^{-2}mol/L$

Putting values in above equation, we get:

$k=\frac{2.303}{60min}\log\frac{1.24\times 10^{-2}}{0.2\times 10^{-2}}\\\\k=0.3041min^{-1}$

Hence, the rate constant for the given reaction is $0.3041min^{-1}$