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Exam 15: Chemical Equilibrium

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Question 41

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Carbon tetrachloride reacts at high temperatures with oxygen to produce two toxic gases, phosgene and chlorine. CCl₄(g) + ¹/₂O₂(g) COCl₂(g) + Cl₂(g) , K_c = 4.4 * 10⁹ at 1,000 K Calculate K_c for the reaction 2CCl₄(g) + O₂(g) 2COCl₂(g) + 2Cl₂(g) .

A) 4.4 * 10⁹
B) 8.8 * 10⁹
C) 1.9 * 10¹⁰
D) 1.9 * 10¹⁹
E) 2.3 * 10^-10

F) A) and D)
G) None of the above

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Question 42

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Consider the chemical reaction 2NH₃(g) N₂(g)+ 3H₂(g). The equilibrium is to be established in a 1.0 L container at 1,000 K, where K_c = 4.0 * 10^-2. Initially, 1,220 moles of NH₃(g)are present. Calculate K_p for the reaction.

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Question 43

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At 700 K, the reaction 2SO₂(g) + O₂(g) 2SO₃(g) has the equilibrium constant K_c = 4.3 * 10⁶, and the following concentrations are present: [SO₂] = 0.010 M; [SO₃] = 10. M; [O₂] = 0.010 M. Is the mixture at equilibrium? If not at equilibrium, in which direction (as the equation is written) , left to right or right to left, will the reaction proceed to reach equilibrium?

The equilibrium constant expression for the reaction CuO(s)+ H₂(g) Cu(s)+ H₂O(g)is K_c = [H₂]/[H₂O].

Consider this reaction at equilibrium at a total pressure P₁: 2SO₂(g) + O₂(g) 2SO₃(g) Suppose the volume of this system is compressed to one-half its initial volume and then equilibrium is reestablished. The new equilibrium total pressure will be

Solid ammonium hydrogen sulfide is introduced into a 2.00-L flask, and the flask is sealed. If this solid decomposes according to the equation NH₄HS(s) NH₃(g) + H₂S(g) , K_p = 0.108 at 25°C, What is the minimum mass of ammonium hydrogen sulfide that must be present in the flask initially if equilibrium is to be established at 25°C?

Which of these situations will result if some CH₄(g) is removed from the reaction CO(g) + 3H₂(g) CH₄(g) + H₂O(g) at equilibrium?

For the following reaction at equilibrium, which choice gives a change that will shift the position of equilibrium to favor formation of more products? 2NOBr(g) 2NO(g) + Br₂(g) , $\Delta$ Hº_rxn = 30 kJ/mol

A solution was prepared such that the initial concentrations of Cu²⁺(aq)and CN^-(aq)were 0.0120 M and 0.0400 M, respectively. These ions react according to the following chemical equation Cu²⁺(aq)+ 4CN^-(aq) Cd(CN)₄^2-(aq)K_c = 1.0 * 10²⁵ What will be the concentration of CN^-(aq)at equilibrium?

The data below refer to the following reaction: 2NO(g)+ Br₂(g) 2NOBr(g) Find the concentration of Br₂ when the system reaches equilibrium.

For the following reaction at equilibrium, which one of the changes below would cause the equilibrium to shift to the left? 2NOBr(g) 2NO(g) + Br₂(g) , $\Delta$ Hº_rxn = 30 kJ/mol

For the following reaction at equilibrium in a reaction vessel, which one of these changes would cause the Br₂ concentration to increase? 2NOBr(g) 2NO(g) + Br₂(g) , $\Delta$ Hº_rxn= 30 kJ/mol

K_c for the reaction CO₂(g)+ H₂(g) H₂O(g)+ CO(g)is 1.6 at about 990ºC. Calculate the number of moles of water in the final equilibrium system obtained by initially adding 1.00 mol of H₂, 2.00 mol of CO₂, 0.750 mol of H₂O, and 1.00 mol of CO to a 5.00 L reactor at 990ºC.

Hydrogen iodide decomposes according to the equation 2HI(g) H₂(g) + I₂(g) , for which K_c = 0.0156 at 400ºC. 0.550 mol HI was injected into a 2.00 L reaction vessel at 400ºC. Calculate the concentration of H₂ at equilibrium.

When the substances in the equation below are at equilibrium, at pressure P and temperature T, the equilibrium can be shifted to favor the products by CuO(s) + H₂(g) H₂O(g) + Cu(s) $\Delta$ Hº_rxn = -2.0 kJ/mol

For the reaction H₂(g)+ I₂(g) 2HI(g), K_P = K_c.

For the reaction at equilibrium 2SO₃ 2SO₂ + O₂ ( $\Delta$ Hº_rxn= 198 kJ/mol) , if we increase the reaction temperature, the equilibrium will

Consider the equilibrium equation C(s)+ H₂O(g)+ 2296 J CO(g)+ H₂(g). Which way will the reaction shift if the pressure on the system is increased?

When the reaction 2O₃(g) 3O₂(g), for which K_p = 3.0 * 10²⁶ at 773ºC, is at equilibrium, the mixture will contain very little O₂ as compared to O₃.

Calcium carbonate decomposes at high temperatures to give calcium oxide and carbon dioxide. CaCO₃(s) CaO(s)+ CO₂(g) K_P for this reaction is 1.16 at 800°C. A 5.00 L vessel containing 10.0 g of CaCO₃(s)was evacuated to remove the air, sealed, and then heated to 800°C. Ignoring the volume occupied by the solid, what will be the overall mass percent of carbon in the solid once equilibrium is reached?