Quesnon 2 oblainat. \begin{tabular}{c|c} \hline HIDM & U/s \\ \hline 1.00 & 0 \\ 0.90 & 100 \\ 0.81 & 200 \\ 0.74 & 300 \\ 0.68 & 400 \\ \hline \end{tabular} 1. Determine graplically, the order of the reaction. 11. What is the rate constant, \( k \), for this reaction? III. Culculate the half-life of the reaction B. For the reaction \[ \begin{array}{l} \text { For the reaction } \\ 5 \mathrm{H}_{2} \mathrm{O}_{2}(\mathrm{aq})+2 \mathrm{Mn}^{2+}(\mathrm{aq}) \longrightarrow 2 \mathrm{MnO}_{4}(\mathrm{aq})+6 \mathrm{H}^{+}(\mathrm{aq})+2 \mathrm{H}_{2} \mathrm{O}(\mathrm{I}) \end{array} \] Determine 1. E Eeil II. \( \Delta G^{6} \)
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Step 1
To determine the order of the reaction graphically, we need to plot the concentration of the reactant (HIDM) against time (U/s). If the plot is a straight line, the reaction is first order. If the plot is a curve that can be linearized by taking the logarithm of Show more…
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The reaction $2 \mathrm{~B} \longrightarrow \mathrm{C}+2 \mathrm{D}$ is found to be zero-order when run at $990^{\circ} \mathrm{C}$. If it takes $3.3 \times 10^{2} \mathrm{~s}$ for an initial concentration of $\mathrm{B}$ to go from $0.50 \mathrm{M}$ to $0.20 \mathrm{M}$, what is the rate constant for the reaction? What is the half-life of the reaction under these conditions?
For the reaction $$ 2 \mathrm{NO}(\mathrm{g})+2 \mathrm{H}_{2}(\mathrm{~g}) \longrightarrow \mathrm{N}_{2}(\mathrm{~g})+2 \mathrm{H}_{2} \mathrm{O}(\mathrm{g}) $$ these data were obtained at $1100 \mathrm{~K}$ : (a) What is the order with respect to NO? With respect to $\mathrm{H}_{2} ?$ (b) What is the overall order? (c) Write the rate law. (d) Calculate the rate constant. (e) Calculate the initial rate of this reaction at $1100 \mathrm{~K}$ when $[\mathrm{NO}]=\left[\mathrm{H}_{2}\right]=8.0 \times 10^{-3} \mathrm{~mol} \mathrm{~L}^{-1}$.
Peroxydisulfate ion, $\mathrm{S}_{2} \mathrm{O}_{8}^{2-}(a q)$ decomposes in aqueous solution according to the equation $$ \begin{aligned} \mathrm{S}_{2} \mathrm{O}_{8}^{2-}(a q)+\mathrm{H}_{2} \mathrm{O}(l) \rightarrow \\ 2 \mathrm{SO}_{4}^{2-}(a q)+\frac{1}{2} \mathrm{O}_{2}(g)+2 \mathrm{H}^{+}(a q) \end{aligned} $$ Given the following data from an experiment with $\left[\mathrm{S}_{2} \mathrm{O}_{8}^{2-}\right]_{0}=0.100 \mathrm{M}$ in a solution with $\left[\mathrm{H}^{+}\right]$ fixed at $0.100 \mathrm{M}$, determine the reaction rate law and calculate the value of the rate constant: \begin{tabular}{cc} \hline$t / \mathrm{min}$ & {$\left[\mathrm{S}_{2} \mathrm{O}_{8}^{2-1} / \mathrm{M}\right.$} \\ \hline 0 & $0.100$ \\ 17 & $0.050$ \\ 34 & $0.025$ \\ 51 & $0.012$ \\ \hline \end{tabular}
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