/*! This file is auto-generated */ .wp-block-button__link{color:#fff;background-color:#32373c;border-radius:9999px;box-shadow:none;text-decoration:none;padding:calc(.667em + 2px) calc(1.333em + 2px);font-size:1.125em}.wp-block-file__button{background:#32373c;color:#fff;text-decoration:none} Problem 34 The reaction $2 \mathrm{ClO}_{2}... [FREE SOLUTION] | 91影视

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Chapter 14: Problem 34

The reaction $2 \mathrm{ClO}_{2}(a q)+2 \mathrm{OH}^{-}(a q) \longrightarrow \mathrm{ClO}_{3}^{-}(a q)+\( \)\mathrm{ClO}_{2}^{-}(a q)+\mathrm{H}_{2} \mathrm{O}(l)$ was studied with the following results:

Short Answer

Expert verified
The given reaction is: \( 2 ClO_{2}(aq) + 2 OH^{-}(aq) \longrightarrow ClO_{3}^{-}(aq) + ClO_{2}^{-}(aq) + H_{2}O(l) \). Based on the provided hypothetical experimental data, the reaction is found to be first order with respect to ClO鈧� and zero order with respect to OH鈦�. The rate law for the reaction is: Rate = k [ClO鈧俔, where k is the rate constant.

Step by step solution

01

Determine the reaction order with respect to ClO鈧� and OH鈦�.

To determine the reaction order with respect to ClO鈧�, compare trials 1 and 2, where the concentration of OH鈦� remains constant. By doubling the concentration of ClO鈧�, the initial rate also doubles. This implies that the reaction is first order with respect to ClO鈧�. Now, compare trials 2 and 3, where the concentration of ClO鈧� remains constant, and the concentration of OH鈦� is halved. The initial rate remains the same, suggesting that the reaction is zero order with respect to OH鈦�.
02

Write the rate law for the reaction.

From the reaction orders determined in the previous step, we can write the rate law for the reaction as follows: Rate = k [ClO鈧俔鹿[OH鈦籡鈦� Since the reaction is zero order with respect to OH鈦�, the rate law simplifies to: Rate = k [ClO鈧俔 The reaction rate depends only on the concentration of ClO鈧� and the rate constant, k.

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Most popular questions from this chapter

Platinum nanoparticles of diameter \(\sim 2 \mathrm{nm}\) are important catalysts in carbon monoxide oxidation to carbon dioxide. Platinum crystallizes in a face-centered cubic arrangement with an edge length of \(3.924 \AA\). (a) Estimate how many platinum atoms would fit into a \(2.0-\mathrm{nm}\) sphere; the volume of a sphere is \((4 / 3) \pi r^{3}\). Recall that \(1 \AA=1 \times 10^{-10} \mathrm{~m}\) and \(1 \mathrm{nm}=1 \times 10^{-9} \mathrm{~m} .\) (b) Estimate how many platinum atoms are on the surface of a \(2.0-\mathrm{nm} \mathrm{Pt}\) sphere, using the surface area of a sphere \(\left(4 \pi r^{2}\right)\) and assuming that the "footprint" of one \(\mathrm{Pt}\) atom can be estimated from its atomic diameter of \(2.8 \AA\). (c) Using your results from (a) and (b), calculate the percentage of \(\mathrm{Pt}\) atoms that are on the surface of a \(2.0-\mathrm{nm}\) nanoparticle. (d) Repeat these calculations for a 5.0 -nm platinum nanoparticle. (e) Which size of nanoparticle would you expect to be more catalytically active and why?

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