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Chapter 1: Problem 49

\(\mathrm{PCl}_{3}(g)+\mathrm{Cl}_{2}(g) \rightarrow \mathrm{PCl}_{5}(g) \Delta H=-92.5 \mathrm{kJ} / \mathrm{mol}\) In which of the following ways could the reaction above be manipulated to create more product? (A) Decreasing the concentration of \(\mathrm{PCl}_{3}\) (B) Increasing the pressure (C) Increasing the temperature (D) None of the above

Short Answer

Expert verified
The correct answer is (B) Increasing the pressure. By Le Chatelier's principle, increasing the pressure will favour the side with fewer moles of gas i.e., the products side (\(PCl_{5}\)), thereby producing more product.

Step by step solution

01

Analyze the Effect of Concentration

Firstly, according to Le Chatelier's principle, if the concentration of the reactants \(PCl_{3}\) or \(Cl_{2}\) is decreased, the equilibrium would shift to the left to compensate for this change. Thus, decreasing the concentration of \(PCl_{3}\) (option A) would not create more product \(PCl_{5}\). It would instead produce less product.
02

Analyze the Effect of Pressure

As for the effect of pressure, according to Le Chatelier's principle, an increase in pressure favors the side of the reaction with fewer moles of gas. In the given reaction: \(PCl_{3}(g)+ Cl_{2}(g) \rightarrow PCl_{5}(g)\), there are two moles of gas on the left and one mole of gas on the right. Therefore, increasing the pressure (option B) would shift the equilibrium to the right (the side with fewer moles of gas), thus producing more \(PCl_{5}\).
03

Analyze the Effect of Temperature

Finally, since the reaction is exothermic (\(\Delta H = -92.5 kJ/mol\)), increasing the temperature (option C) would add more heat to the system. According to Le Chatelier's principle, this would cause the system to counteract this change by moving in the direction that absorbs heat. In this case, that direction is the reverse reaction (to the left), which would consequently form less product (\(PCl_{5}\)). So, increasing the temperature would not create more product.

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Most popular questions from this chapter

1.50 g of \(\mathrm{NaNO}_{3}\) is dissolved into 25.0 \(\mathrm{mL}\) of water, causing the temperature to increase by \(2.2^{\circ} \mathrm{C}\) . The density of the final solution is found to be 1.02 \(\mathrm{g} / \mathrm{mL}\) . Which of the following expressions will correctly calculate the heat gained by the water as the NaNO, dissolves? Assume the volume of the solution remains unchanged. (A) \((25.0)(4.18)(2.2)\) (B) \(\frac{(26.5)(4.18)(2.2)}{1.02}\) (C) \(\frac{(1.02)(4.18)(2.2)}{1.50}\) (D) \((25.0)(1.02)(4.18)(2.2)\)

A strong acid/strong base titration is completed using an indicator which changes color at the exact equivalence point of the titration. The protonated form of the indicator is HIn, and the deprotonated form is In. At the equivalence point of the reaction: (A) \([\mathrm{HIn}]=\left[\mathrm{In}^{-}\right]\) (B) \([\mathrm{HIn}]=1 /\left[\mathrm{In}^{-}\right]\) (C) \([\mathrm{HIn}]=2\left[\mathrm{In}^{-}\right]\) (D) \([\mathrm{HIn}]=\left[\mathrm{In}^{-}\right]^{2}\)

\(2 \mathrm{HI}(g)+\mathrm{Cl}_{2}(g) \rightleftharpoons 2 \mathrm{HCl}(g)+\mathrm{I}_{2}(g)+\) energy A gaseous reaction occurs and comes to equilibrium, as shown above. Which of the following changes to the system will serve to increase the number of moles of \(\mathrm{I}_{2}\) present at equilibrium? (A) Increasing the volume at constant temperature (B) Decreasing the volume at constant temperature (C) Increasing the temperature at constant volume (D) Decreasing the temperature at constant volume

Nitrogen’s electronegativity value is between those of phosphorus and oxygen. Which of the following correctly describes the relationship between the three values? (A) The value for nitrogen is less than that of phosphorus because nitrogen is larger, but greater than that of oxygen because nitrogen has a greater effective nuclear charge. (B) The value for nitrogen is less than that of phosphorus because nitrogen has fewer protons, but greater than that of oxygen because nitrogen has fewer valence electrons. (C) The value for nitrogen is greater than that of phosphorus because nitrogen has fewer electrons, but less than that of oxygen because nitrogen is smaller. (D) The value for nitrogen is greater than that of phosphorus because nitrogen is smaller, but less than that of oxygen because nitrogen has a smaller effective nuclear charge.

The following reaction is found to be at equilibrium at 25°C: \(2 \mathrm{SO}_{3}(g) \leftrightarrow \mathrm{O}_{2}(g)+2 \mathrm{SO}_{2}(g) \quad \Delta H=-198 \mathrm{kJ} / \mathrm{mol}\) The solubility product, \(K_{s p}\) , of \(\mathrm{AgCl}\) is \(1.8 \times 10^{-10}\) . Which of the following expressions is equal to the solubility of \(\mathrm{AgCl}\)? (A) \(\left(1.8 \times 10^{-10}\right)^{2}\) molar (B) \(\frac{1.8 \times 10^{-10}}{2}\) molar (C) \(1.8 \times 10^{-10}\) molar (D) \(\sqrt{1.8 \times 10^{-10}}\) molar
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