Respuesta :
Explanation:
[tex]2 N_2O_5(g)\rightarrow 4 NO_2(g)+O_2(g)[/tex]
Rate of the reaction ,k= [tex]3.38\times 10^{-5} s^{-1}[/tex]
Half life of the [tex]N_2O_5=t_{\frac{1}{2}}[/tex]
[tex]t_{\frac{1}{2}}=\frac{0.693}{k}=\frac{0.693}{3.38\times 10^{-5} s^{-1}}[/tex](first order kinetics)
[tex]t_{\frac{1}{2}}=20,502.958 seconds[/tex]
Half life of the [tex]N_2O_5[/tex] is 20,502.958 seconds.
Integrated rate equation for first order kinetics in gas phase is given as:
[tex]k=\frac{2.303}{t}\log\frac{p_o}{2p_o-p}[/tex]
p= pressure of the gas at given time t.
[tex]p_o[/tex] = Initial pressure of the gas
(i) When, t = 50 sec
[tex]p_o=500 torr[/tex]
[tex]3.38\times 10^{-5} s^{-1}=\frac{2.303}{50 s}\log\frac{500 Torr}{2(500 Torr)-p}[/tex]
p = 500.49 Torr
(ii)When, t = 20 min = 1200 sec
[tex]p_o=500 torr[/tex]
[tex]3.38\times 10^{-5} s^{-1}=\frac{2.303}{1200 s}\log\frac{500 Torr}{2(500 Torr)-p}[/tex]
p = 519.83 Torr
