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Chapter 2: Problem 24

For each of the questions, four choices have been provided. Select the correct alternative. Equilibrium position of which of the following reactions is not affected by change in pressure? (a) \(\mathrm{I}_{2(\mathrm{~s})}+5 \mathrm{~F}_{2(\mathrm{~g})} \rightarrow 2 \mathrm{IF}_{5(\mathrm{~g})}\) (b) \(\mathrm{FeO}_{(\mathrm{s})}+\mathrm{CO}_{(\mathrm{g})} \rightarrow \mathrm{Fe}_{(\mathrm{s})}+\mathrm{CO}_{(\mathrm{g})}\) (c) \(2 \mathrm{Cu}\left(\mathrm{NO}_{3}\right)_{2(\mathrm{~s})} \rightarrow 2 \mathrm{CuO}_{(\mathrm{s})}+4 \mathrm{NO}_{2(\mathrm{~g})}+\mathrm{O}_{2(\mathrm{~g})}\) (d) \(\mathrm{N}_{2} \mathrm{O}_{4(\mathrm{~g})} \rightarrow 2 \mathrm{NO}_{2(\mathrm{~g})}\)

Short Answer

Expert verified
Answer: (b) FeO(s) + CO(g) → Fe(s) + CO(g)

Step by step solution

01

Examine reaction (a)

Compare the total moles of gaseous reactants and products in the equation: \(I_2(s) + 5F_2(g) \rightarrow 2IF_5(g)\) On the left side, we have 5 moles of gaseous \(F_2\). On the right side, we have 2 moles of gaseous \(IF_5\). The number of moles of gaseous species is different, thus pressure change will affect this reaction's equilibrium position.
02

Examine reaction (b)

Compare the total moles of gaseous reactants and products in the equation: \(FeO(s) + CO(g) \rightarrow Fe(s) + CO(g)\) On the left side, we have 1 mole of gaseous \(CO\). On the right side, we also have 1 mole of gaseous \(CO\). The number of moles of gaseous species is the same, thus pressure change won't affect this reaction's equilibrium position. It appears we have found the correct answer, but for completeness, let's examine the remaining reactions.
03

Examine reaction (c)

Compare the total moles of gaseous reactants and products in the equation: \(2Cu(NO_3)_2(s) \rightarrow 2CuO(s) + 4NO_2(g) + O_2(g)\) Reactants have no gaseous component. On the right side, we have 4 moles of gaseous \(NO_2\) and 1 mole of gaseous \(O_2\). The number of moles of gaseous species is different on each side, thus pressure change will affect this reaction's equilibrium position.
04

Examine reaction (d)

Compare the total moles of gaseous reactants and products in the equation: \(N_2O_4(g) \rightarrow 2NO_2(g)\) On the left side, we have 1 mole of gaseous \(N_2O_4\). On the right side, we have 2 moles of gaseous \(NO_2\). The number of moles of gaseous species is different, thus pressure change will affect this reaction's equilibrium position. Thus, the correct alternative is (b), where the equilibrium position of the reaction is not affected by changes in pressure.

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Most popular questions from this chapter

For each of the questions, four choices have been provided. Select the correct alternative. For a reaction \(\mathrm{A}+\mathrm{B} \rightarrow \mathrm{C}\), the rate law is written as \(\mathrm{r}=\mathrm{k}[\mathrm{A}]^{2}[\mathrm{~B}] .\) Doubling the concentration of "A" without changing concentration of "B" increases the rate of reaction by (a) 2 times (b) 4 times (c) 8 times (d) 16 times

If the rate with respect to \(\mathrm{O}_{2}, \mathrm{NO}\) and \(\mathrm{NO}_{2}\) are respectively $$ \frac{-\Delta\left[\mathrm{O}_{2}\right]}{\Delta \mathrm{t}}, \frac{-1}{2}, \frac{\Delta[\mathrm{NO}]}{\Delta \mathrm{t}}, \frac{+1}{2} \frac{\Delta\left[\mathrm{NO}_{2}\right]}{\Delta \mathrm{t}} $$ then the corresponding chemical equation is \(2 \mathrm{NO}\) \(+\mathrm{O}_{2} \rightarrow 2 \mathrm{NO}_{2}\)

For each of the questions, four choices have been provided. Select the correct alternative. If \(\mathrm{r}=\frac{-3}{2} \frac{\Delta[\mathrm{A}]}{\Delta \mathrm{t}}=\frac{-5}{2} \frac{\Delta[\mathrm{B}]}{\Delta \mathrm{t}}=\frac{+7}{3} \frac{[\Delta \mathrm{C}]}{\Delta \mathrm{t}}\), which of the following is the corresponding reaction? (a) \(2 / 3 \mathrm{~A}+2 / 5 \mathrm{~B} \rightarrow 3 / 7 \mathrm{C}\) (b) \(2 / 3 \mathrm{~A}+5 / 2 \mathrm{~B} \rightarrow 7 / 3 \mathrm{C}\) (c) \(3 / 2 \mathrm{~A}+5 / 2 \mathrm{~B} \rightarrow 7 / 3 \mathrm{C}\) (d) \(7 / 3 \mathrm{C}+5 / 2 \mathrm{~B} \rightarrow 3 / 2 \mathrm{~A}\)

For each of the questions, four choices have been provided. Select the correct alternative. The equilibrium constant for the given reaction, \(\mathrm{CaCO}_{3(\mathrm{~s})} \mathrm{CaO}_{(\mathrm{s})}+\mathrm{CO}_{2}(\mathrm{~g})\) is given by (a) \(\mathrm{K}_{\mathrm{c}}=\frac{[\mathrm{CaO}] \cdot\left[\mathrm{CO}_{2}\right]}{\left[\mathrm{CaCO}_{3}\right]}\) (b) \(\mathrm{K}_{\mathrm{c}}=\frac{[\mathrm{CaO}]}{\left[\mathrm{CaCO}_{3}\right]}\) (c) \(\mathrm{K}_{\mathrm{c}}=\left[\mathrm{CO}_{2}\right]\) (d) \(\mathrm{K}_{\mathrm{c}}=\frac{[\mathrm{CaO}]}{\left[\mathrm{CO}_{2}\right]}\)

For each of the questions, four choices have been provided. Select the correct alternative. According to Le Chatelier's principle, (a) an increase in pressure always causes a change in position of equilibrium for any reaction (b) the yield of \(\mathrm{NH}_{3}\) decreases from its constituents at lower temperature (c) an increase in temperature causes a decrease in the value of \(\mathrm{K}_{\mathrm{c}}\) for an exothermic reaction (d) the \(\mathrm{K}_{\mathrm{c}}\) is decreased for the reaction \(\mathrm{A}_{(\mathrm{s})}+\mathrm{B}_{(\mathrm{g})}\) \(\rightarrow \mathrm{C}_{(\mathrm{g})}\), if the concentration of \(\mathrm{A}\) is increased
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