3. For the reaction ( 2 mathrm{H}_{2} mathrm{O}_{2}(a q) ightarrow 2 mathrm{H}_{2} mathrm{O}(l)+mathrm{O}_{2}(g) ), the following data were collected at constant temperature: egin{tabular}{|l|l|} hline Time ( (mathrm{s}) ) & {( left[mathrm{H}_{2} mathrm{O}_{2} ight](mathrm{mol} / mathrm{L}) )} \ hline 0 & 1.000 \ hline ( 2.16 imes 10^{4} ) & 0.500 \ hline ( 4.32 imes 10^{4} ) & 0.250 \ hline end{tabular} a) Calculate the average rate of decomposition of ( mathrm{H}_{2} mathrm{O}_{2} ) between 0 and ( 2.16 imes 10^{4} mathrm{~s} ). b) Use your answer to calculate the average rate of production of ( mathrm{O}_{2} ) over the same time period.
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The reaction given is the decomposition of hydrogen peroxide (H2O2) into water (H2O) and oxygen (O2). The question asks for the average rate of decomposition of H2O2 and the average rate of production of O2 over a specific time period. Show more…
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At $40^{\circ} \mathrm{C}, \mathrm{H}_{2} \mathrm{O}_{2}(a q)$ will decompose according to the following reaction: $$2 \mathrm{H}_{2} \mathrm{O}_{2}(a q) \longrightarrow 2 \mathrm{H}_{2} \mathrm{O}(l)+\mathrm{O}_{2}(g)$$ The following data were collected for the concentration of $\mathrm{H}_{2} \mathrm{O}_{2}$ at various times. a. Calculate the average rate of decomposition of $\mathrm{H}_{2} \mathrm{O}_{2}$ between 0 and $2.16 \times 10^{4}$ s. Use this rate to calculate the average rate of production of $\mathrm{O}_{2}(g)$ over the same time period. b. What are these rates for the time period $2.16 \times 10^{4} \mathrm{s}$ to $4.32 \times 10^{4} \mathrm{s} ?$
At $40^{\circ} \mathrm{C}, \mathrm{H}_{2} \mathrm{O}_{2}(a q)$ will decompose according to the following reaction: $$ 2 \mathrm{H}_{2} \mathrm{O}_{2}(a q) \longrightarrow 2 \mathrm{H}_{2} \mathrm{O}(l)+\mathrm{O}_{2}(\mathrm{~g}) $$ The following data were collected for the concentration of $\mathrm{H}_{2} \mathrm{O}_{2}$ at various times. $$ \begin{array}{|cc|} \hline \begin{array}{c} \text { Time } \\ (\mathbf{s}) \end{array} & \begin{array}{c} {\left[\mathrm{H}_{2} \mathrm{O}_{2}\right]} \\ (\mathrm{mol} / \mathrm{L}) \end{array} \\ \hline 0 & 1.000 \\ \hline 2.16 \times 10^{4} & 0.500 \\ \hline 4.32 \times 10^{4} & 0.250 \\ \hline \end{array} $$ a. Calculate the average rate of decomposition of $\mathrm{H}_{2} \mathrm{O}_{2}$ between 0 and $2.16 \times 10^{4} \mathrm{~s}$. Use this rate to calculate the average rate of production of $\mathrm{O}_{2}(g)$ over the same time period. b. What are these rates for the time period $2.16 \times 10^{4} \mathrm{~s}$ to $4.32 \times 10^{4} \mathrm{~s} ?$
At 40°C, H2O2(aq) will decompose according to the following reaction: 2H2O2(aq) ---> 2H2O(l) + O2(g). The following data were collected for the concentration of H2O2 at various times. Time: H2O2 (mol/L) 0 1.100 2.53 x 10^4 0.488 5.06 x 10^4 0.217 a. Calculate the average rate of decomposition of H2O2 between 0 and 2.53 x 10^4 s. (Use this rate to calculate the average rate of production of O2(g) over the same time period.) b. What are these rates for the time period 2.53 x 10^4 s to 5.06 x 10^4 s? 2. A certain first-order reaction is 54% complete in 85 s. What are the values of the rate constant and the half-life for this process?
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