The decomposition of N2 O5 (g) longrightarrow NO2 (g) + NO3 (g) proceeds as a first order reaction with a half-life period of 30 s at a certain temperature. If the initial concentration [N2 O5] = 0.4 M, what is the rate constant of the reaction?

Question

The decomposition of N2 O5 (g) longrightarrow NO2 (g) + NO3 (g) proceeds as a first order reaction with a half-life period of 30 s at a certain temperature. If the initial concentration [N2 O5] = 0.4 M, what is the rate constant of the reaction? (A) 0.00924 s-1 (B) 0.0231 s-1 (C) 75 s-1 (D) 12 s-1

Tardigrade Admin · Accepted Answer

For a first order reaction k = (0.693/t1/2) = (0.693/30) = 0.0231 s-1

Q. The decomposition of $N_{2} O_{5} (g) ⟶ N O_{2} (g) + N O_{3} (g)$ proceeds as a first order reaction with a half-life period of $30 s$ at a certain temperature. If the initial concentration $[N_{2} O_{5}] = 0.4 M$ , what is the rate constant of the reaction?

$0.00924 s^{- 1}$

$0.0231 s^{- 1}$

$75 s^{- 1}$

$12 s^{- 1}$

For a first order reaction
$k = \frac{0.693}{t _{1/2}} = \frac{0.693}{30} = 0.0231 s^{- 1}$

Q. The decomposition of N2​O5​(g)⟶NO2​(g)+NO3​(g) proceeds as a first order reaction with a half-life period of 30s at a certain temperature. If the initial concentration [N2​O5​]=0.4M, what is the rate constant of the reaction?

0.00924s−1

0.0231s−1

75s−1

12s−1