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  •  Consider the reaction <img alt="\mathrm{A (g) \longrightarrow B(g)+C(g)}" src="https://entrancecorner.oncodecogs.com/gif.latex?%5Cmathrm%7BA%20%28g%29%20%5Clongrightarrow%20B%28g%29&am

 Consider the reaction
\mathrm{A (g) \longrightarrow B(g)+C(g)}.  If the initial pressure of \mathrm{A } is \mathrm{180 \mathrm{~mm}\, Hg} and the total pressure at the end of \mathrm{30\, \mathrm{min}\, } is \mathrm{240\, \mathrm{mm}\,Hg } what will be the half life of the reaction if it follows first order kinetics.

Option: 1

15 min


Option: 2

40 min


Option: 3

51 min


Option: 4

70 min


Answers (1)

best_answer

           \mathrm{A(g) \longrightarrow B(g)+C(g)}
\mathrm{t= 0 \quad p_{0}}                 0             0
\mathrm{t= t \quad p_{0}-x \quad \: \: n \quad \quad x}

\mathrm{P_{\text {Total }} =P_{0}-x+x+x=P_{0}+x }
\mathrm{P_{T} =P_{0}+x \Rightarrow 240=180+x }

\mathrm{x=240-180=60 }.

for first order reaction
\mathrm{k=\frac{2.303}{t} \log \left(\frac{p_{0}}{p_{0}-x}\right)=\frac{2.303}{30} \log \left(\frac{180}{180-60}\right) }
\mathrm{ t_{1 / 2}=\frac{2.303 \times \log (2)}{k}=\frac{2.303 \times 0.3 \times 30}{2303 \times \log (3 / 2)} }
\mathrm{ t_{1 / 2} = 51 \mathrm{~min} }.

Posted by

Anam Khan

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