3. Nitrous acid slowly decomposes ( \( 298 \mathrm{~K}) \) according to the following balanced chemical reaction: * for graphing integrated eq
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Nitrous acid slowly decomposes to $\mathrm{NO}, \mathrm{NO}_{2},$ and water in the following second-order reaction: $$ 2 \mathrm{HNO}_{2}(a q) \rightarrow \mathrm{NO}(g)+\mathrm{NO}_{2}(g)+\mathrm{H}_{2} \mathrm{O}(\ell) $$ a. Use the data in the table to determine the rate constant for this reaction at $298 \mathrm{K}$ $$\begin{array}{cc} \text { Time (min) } & {\left[\mathrm{HNO}_{2}\right](\mu M)} \\ 0.0 & 0.1560 \\ \hline 1000.0 & 0.1466 \\ \hline 1500.0 & 0.1424 \\ \hline 2000.0 & 0.1383 \\ \hline 2500.0 & 0.1345 \\ \hline 3000.0 & 0.1309 \\ \hline \end{array}$$ b. Determine the half-life for the decomposition of $\mathrm{HNO}_{2}.$
Write out the stepwise $K_{\mathrm{a}}$ reactions for the diprotic acid $\mathrm{H}_{2} \mathrm{SO}_{3}$
Nitrous acid slowly decomposes to $\mathrm{NO}, \mathrm{NO}_{2},$ and water in the following second-order reaction: $$2 \mathrm{HNO}_{2}(a q) \rightarrow \mathrm{NO}(g)+\mathrm{NO}_{2}(g)+\mathrm{H}_{2} \mathrm{O}(\ell)$$ a. Use the following data to determine the rate constant for this reaction at $298 \mathrm{K}:$ $$\begin{array}{cc} \text { Time (min) } & {\left[\mathrm{HNO}_{2}\right](\mu M)} \\0 & 0.1560 \\\hline 1000 & 0.1466 \\\hline 1500 & 0.1424 \\\hline 2000 & 0.1383 \\\hline 2500 & 0.1345 \\\hline 3000 & 0.1309 \\\hline\end{array}$$ b. Determine the half-life for the decomposition of $\mathrm{HNO}_{2}$. c. If the experiment that yielded the results in the preceding table had been continued for 3000 minutes more, what would the concentration of HNO $_{2}$ have been?
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