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(A) The reaction is $2 A_{(g)} \rightarrow B_{(g)} + C_{(s)}$.Let the initial pressure of $A$ be $P_0$.At $t = \infty$ (completion),only $B_{(g)}$ is

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$0.0693$

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(A) The reaction is $2 A_{(g)} ightarrow B_{(g)} + C_{(s)}$.Let the initial pressure of $A$ be $P_0$.At $t = \infty$ (completion),only $B_{(g)}$ is present,so $P_B = P_0 / 2 = 200 \ Pa$,which means $P_0 = 400 \ Pa$.At $t = 10 \ min$,let the pressure of $A$ reacted be $2x$.Initial: $P_A = 400, P_B = 0, P_C = 0$.At $t = 10$: $P_A = 400 - 2x, P_B = x, P_C = 0$ (since $C$ is solid).Total pressure $P_t = (400 - 2x) + x = 400 - x = 300 \ Pa$.Therefore,$x = 100 \ Pa$.The partial pressure of $A$ at $t = 10 \ min$ is $P_A = 400 - 2(100) = 200 \ Pa$.For a first-order reaction,$k = \frac{2.303}{t} \log \left( \frac{P_0}{P_A} ight)$.$k = \frac{2.303}{10} \log \left( \frac{400}{200} ight) = \frac{2.303}{10} \log 2$.$k = \frac{2.303 	imes 0.3010}{10} \approx 0.0693 \ min^{-1}$.

$S$.no.	Time	Total pressure in Pascal
$1.$	At the end of $10 \ min$	$300$
$2.$	After completion	$200$

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The following data were obtained during the first-order decomposition of $2 A_{(g)} \rightarrow B_{(g)} + C_{(s)}$ at a constant volume and at a particular temperature. The rate constant in $min^{-1}$ is:$S$.no.TimeTotal pressure in Pascal$1.$At the end of $10 \ min$$300$$2.$After completion$200$