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Chapter 13: Problem 71

Suppose the reaction system $$\mathrm{UO}_{2}(s)+4 \mathrm{HF}(g) \rightleftharpoons \mathrm{UF}_{4}(g)+2 \mathrm{H}_{2} \mathrm{O}(g)$$ has already reached equilibrium. Predict the effect that each of the following changes will have on the equilibrium position. Tell whether the equilibrium will shift to the right, will shift to the left, or will not be affected. a. Additional \(\mathrm{UO}_{2}(s)\) is added to the system. b. The reaction is performed in a glass reaction vessel; HF \((g)\) attacks and reacts with glass. c. Water vapor is removed.

Short Answer

Expert verified
a. The equilibrium will not be affected since the added UO2(s) as a solid does not directly influence the equilibrium. b. The equilibrium will shift to the left due to the reaction of HF(g) with the glass, decreasing its concentration and causing the system to respond by converting more UF4(g) and H2O(g) into UO2(s) and HF(g). c. The equilibrium will shift to the right as a result of water vapor removal, with the system attempting to counteract the decrease in H2O(g) concentration by converting more UO2(s) and HF(g) into UF4(g) and H2O(g).

Step by step solution

01

a. Effect of adding additional UO2(s) to the reaction system

When additional UO2(s) is added to the system, it increases the concentration of UO2(s). However, since it is a solid, its concentration does not affect the equilibrium directly. Consequently, the equilibrium position will not be affected, and there will be no shift in the equilibrium.
02

b. Effect of HF(g) reacting with glass

When HF(g) reacts with the glass, it effectively removes some of the HF(g) from the reaction system, resulting in a decreased concentration of HF(g). According to Le Chatelier's Principle, the system will respond by trying to increase the concentration of HF(g) back to its previous level. To do this, the reaction will shift to the left, converting more UF4(g) and H2O(g) into UO2(s) and HF(g).
03

c. Effect of removing water vapor

When water vapor (H2O(g)) is removed from the system, its concentration decreases. Following Le Chatelier's Principle, the system will attempt to counteract this by increasing the concentration of H2O(g). In order to do this, the reaction will shift to the right, converting more UO2(s) and HF(g) into UF4(g) and H2O(g).

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Most popular questions from this chapter

At high temperatures, elemental nitrogen and oxygen react with each other to form nitrogen monoxide: $$\mathrm{N}_{2}(g)+\mathrm{O}_{2}(g) \rightleftharpoons 2 \mathrm{NO}(g)$$ Suppose the system is analyzed at a particular temperature, and the equilibrium concentrations are found to be \(\left[\mathrm{N}_{2}\right]=\) \(0.041 M,\left[\mathrm{O}_{2}\right]=0.0078 M,\) and $[\mathrm{NO}]=4.7 \times 10^{-4} M .\( Calculate the value of \)K$ for the reaction.

At \(35^{\circ} \mathrm{C}, K=1.6 \times 10^{-5}\) for the reaction $$2 \mathrm{NOCl}(g) \rightleftharpoons 2 \mathrm{NO}(g)+\mathrm{Cl}_{2}(g)$$ Calculate the concentrations of all species at equilibrium for each of the following original mixtures. a. 2.0 moles of pure \(\mathrm{NOCl}\) in a 2.0 \(\mathrm{L}\) flask b. 1.0 mole of NOCl and 1.0 mole of NO in a 1.0 - flask c. 2.0 moles of \(\mathrm{NOCl}\) and 1.0 mole of \(\mathrm{Cl}_{2}\) in a \(1.0-\mathrm{L}\) flask

An important reaction in the commercial production of hydrogen is $$\mathrm{CO}(g)+\mathrm{H}_{2} \mathrm{O}(g) \rightleftharpoons \mathrm{H}_{2}(g)+\mathrm{CO}_{2}(g)$$ How will this system at equilibrium shift in each of the five following cases? a. Gaseous carbon dioxide is removed. b. Water vapor is added. c. In a rigid reaction container, the pressure is increased by adding helium gas. d. The temperature is increased (the reaction is exothermic). e. The pressure is increased by decreasing the volume of the reaction container.

At \(25^{\circ} \mathrm{C}, K=0.090\) for the reaction $$\mathrm{H}_{2} \mathrm{O}(g)+\mathrm{Cl}_{2} \mathrm{O}(g) \rightleftharpoons 2 \mathrm{HOCl}(g)$$ Calculate the concentrations of all species at equilibrium for each of the following cases. a. 1.0 \(\mathrm{g} \mathrm{H}_{2} \mathrm{O}\) and 2.0 $\mathrm{g} \mathrm{Cl}_{2} \mathrm{O}$ are mixed in a 1.0 -L flask. b. 1.0 mole of pure HOCl is placed in a 2.0 \(\mathrm{L}\) flask.

The following equilibrium pressures at a certain temperature were observed for the reaction $$\begin{aligned} 2 \mathrm{NO}_{2}(g) & \rightleftharpoons 2 \mathrm{NO}(g)+\mathrm{O}_{2}(g) \\ P_{\mathrm{NO}_{2}} &=0.55 \mathrm{atm} \\\ P_{\mathrm{NO}} &=6.5 \times 10^{-5} \mathrm{atm} \\ P_{\mathrm{O}_{2}} &=4.5 \times 10^{-5} \mathrm{atm} \end{aligned}$$ Calculate the value for the equilibrium constant \(K_{\mathrm{p}}\) at this temperature.
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