Numerade

Questions asked

INSTANT ANSWER

Q9. The rate of the second-order decomposition of acetaldehyde \( \left(\mathrm{CH}_{3} \mathrm{CHO}\right) \) was measured over the temperature range \( 700-1000 \mathrm{~K} \), and the rate constants are reported below. \begin{tabular}{|l|l|l|l|l|l|l|l|l|} \hline \( \mathbf{T} / \mathbf{K} \) & 700 & 740 & 780 & 800 & 810 & 850 & 950 & 1000 \\ \hline \( \mathbf{k} /\left(\mathbf{d m}^{3} \mathbf{m o l}^{-1} \mathbf{S}^{-1}\right) \) & \( 0.007 \) & \( 0.041 \) & \( 0.209 \) & \( 0.446 \) & \( 0.642 \) & \( 2.540 \) & \( 47.59 \) & \( 165.34 \) \\ \hline \end{tabular} 1. Show the plot. 2. Write down the equation. 3. Find \( \mathrm{E}_{2} \) and \( \mathrm{A} \).

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INSTANT ANSWER

Q8. The gas-phase reaction of fluorine atoms with bromine is shown below. \[ \mathrm{F}+\mathrm{Br}_{2} \rightarrow \mathrm{FBr}+\mathrm{Br} \] The following concentrations of \( \mathrm{Br}_{2} \) were observed as a function of time at \( 298 \mathrm{~K} \) when the initial fluorine atom concentration was \( [\mathrm{F}]=4 \times 10^{-9} \mathrm{~mol} \mathrm{dm}^{-3} \). \begin{tabular}{|c|c|} \hline Time/s & {\( \left[\mathbf{B r}_{2}\right] / \mathbf{1 0}^{-9} \mathbf{m o l ~ d m}^{-\mathbf{3}} \)} \\ \hline 0 & \( 0.16 \) \\ \hline \( 1.05 \) & \( 0.106 \) \\ \hline \( 1.95 \) & \( 0.077 \) \\ \hline \( 4.05 \) & \( 0.035 \) \\ \hline \( 5.85 \) & \( 0.018 \) \\ \hline \end{tabular} Knowing that the order with respect to \( F \) is 1 a) Write down the rate equation and calculate the rate constant. b) What is the overall order? c) What is the molecularity of the reaction?

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INSTANT ANSWER

Q7. The data below is provided for the following reaction \( \mathrm{A} \rightarrow \mathrm{P} \) \begin{tabular}{|c|c|} \hline Time (s) & [A] \( \mathbf{m o l} / \mathbf{d m}^{\mathbf{3}} \) \\ \hline 0 & \( 1.00 \) \\ \hline 15 & \( 0.92 \) \\ \hline 20 & \( 0.90 \) \\ \hline 50 & \( 0.78 \) \\ \hline 75 & \( 0.71 \) \\ \hline 105 & \( 0.63 \) \\ \hline 130 & \( 0.58 \) \\ \hline 150 & \( 0.55 \) \\ \hline \end{tabular} 1. Find out whether the reaction is \( 0^{\text {th }}, 1^{\text {st }} \), or \( 2^{\text {nd }} \) order. Show your calculations and plots for each case. 2. What is the order of the reaction? 3. What is the value of rate constant \( (\mathrm{k}) \) ? 4. Write down the rate equation. 5. Determine \( [\mathrm{A}] \) at \( 90 \mathrm{~s} \).

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INSTANT ANSWER

Q6. The experimental results of the decomposition of ethylene oxide: are presented in the following table: 1. What is the initial pressure of the reaction? 2. Prove that the reaction is first order using a graph that you can draw based on the given data. 3. Calculate the rate constant \( (\mathrm{k}) \) 4. What is the half-life time of this reaction?

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Deniz O.