Gaseous N_2O_5 (g) decomposes according to the following equation : N_2O_5 (g) → 2NO (g)+1/2 O_2 (g) The experimental rate law is - Δ [N_2O_5]\/\Deltat = k[N_0O_5]. At a certain temperature the rate constant is k = 5.0 \times 10^{-4} s^{-1}. In how many seconds will be the concentration of N_0O_5 decrease to one-tenth of its initial value?

Correct Answer is : 4.6 × 103 s

UPSEE Solved Model Paper 1

Question : 88 of 150

Marks: +1, -0

Gaseous N2O5 (g) decomposes according to the following equation :
N2O5(g) → 2NO(g)+

O2(g)
The experimental rate law is - Δ [N2O5]∕Δt = k[N0O5]. At a certain temperature the rate constant is k = 5.0×10−4s−1. In how many seconds will be the concentration of N0O5 decrease to one-tenth of its initial value?

2.0 × 103 s
4.6 × 103 s
2.1 × 102 s
1.4 × 103 s

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