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(B) For the decomposition of ammonium nitrate $(NH_4NO_2 \rightarrow N_2 + 2H_2O)$, the volume of $N_2$ gas evolved at time $t$ $(V_t)$ is proportiona

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(B) For the decomposition of ammonium nitrate $(NH_4NO_2 \rightarrow N_2 + 2H_2O)$, the volume of $N_2$ gas evolved at time $t$ $(V_t)$ is proportional to the amount of reactant consumed.The rate constant $K$ for a first-order reaction is given by the formula: $K = \frac{2.303}{t} \log \frac{V_{\infty}}{V_{\infty} - V_t}$.Substituting the given values ($V_{\infty} = 35.05$ $cc$) into the equation for different time intervals yields a constant value for $K$.Since the data fits the first-order integrated rate equation, the order of the reaction is $1$.

$N_2$ volume in $cc$ $(V_t)$	$6.25$	$9.50$	$11.42$	$13.65$	$35.05$ $(V_{\infty})$
Time $(t)$ in minutes	$10$	$15$	$20$	$25$	$\infty$

The following data are for the decomposition of ammonium nitrate in aqueous solution. The order of the reaction is:
$N_2$ volume in $cc$ $(V_t)$ $6.25$ $9.50$ $11.42$ $13.65$ $35.05$ $(V_{\infty})$
Time $(t)$ in minutes $10$ $15$ $20$ $25$ $\infty$

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The following data are for the decomposition of ammonium nitrate in aqueous solution. The order of the reaction is:$N_2$ volume in $cc$ $(V_t)$$6.25$$9.50$$11.42$$13.65$$35.05$ $(V_{\infty})$Time $(t)$ in minutes$10$$15$$20$$25$$\infty$