In the reaction 2N2O5 → 4NO2 +O2 initial pressure is 500 atm and rate constant K is 3.38 × 10-5 sec-1. After 10 minutes the final pressure of N2O5 is

Question

In the reaction 2N2O5 → 4NO2 +O2 initial pressure is 500 atm and rate constant K is 3.38 × 10-5 sec-1. After 10 minutes the final pressure of N2O5 is (A) 490 atm (B) 250 atm (C) 480 atm (D) 420 atm

Tardigrade Admin · Accepted Answer

P0=500 atm K=(2.303/t) log(P0/P1) 3.38×10-5=(2.303/10×60)log(500/Pt) or 0.00880=log(500/Pt)⇒ (500/1.02)=490 atm

Q. In the reaction $2 N_{2} O_{5} \to 4 N O_{2} + O_{2}$ initial pressure is $500$ atm and rate constant $K$ is $3.38 \times 1 0^{- 5} se c^{- 1.}$ After 10 minutes the final pressure of $N_{2} O_{5}$ is

$490$ atm

$250$ atm

$480$ atm

$420$ atm

$P_{0} = 500 a t m$
$K = \frac{2.303}{t} l o g \frac{P _{0}}{P _{1}}$
$3.38 \times 1 0^{- 5} = \frac{2.303}{10 \times 60} l o g \frac{500}{P _{t}}$
or $0.00880 = l o g \frac{500}{P _{t}} \Rightarrow \frac{500}{1.02} = 490 a t m$

Q. In the reaction 2N2​O5​→4NO2​+O2​ initial pressure is 500 atm and rate constant K is 3.38×10−5sec−1. After 10 minutes the final pressure of N2​O5​ is

490 atm

250 atm

480 atm

420 atm