# ChemWksht - A mixture of 1.0 g H2 and 1.06 g H2S in a...

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A mixture of 1.0 g H 2 and 1.06 g H 2 S in a 0.500-L flask comes to equilibrium at 1670 K: 2H 2 (g) + S 2 (g) ↔ 2H 2 S(g). The equilibrium amount of S 2 (g) found is 8.00 *10 -6 mol. Determine the value of K p at 1670 K. 1. At 2000 K, K c = 0.154 for the reaction 2 CH 4 (g) ↔ C 2 H 2 (g) + 3H 2 (g). If a 1.00-L equilibrium mixture at 2000 K contains 0.10 mol each of CH 4 (g) and H 2 (g), a. What is the mole fraction of C 2 H 2 (g) present? b. Is the conversion of CH 4 (g) to C 2 H 2 (g) favored at high or low pressures? c. If the equilibrium mixture at 2000 K is transferred from a 1.00-L flask to a 2.00-L flask, will the number of moles of C 2 H 2 (g) increase, decrease, or remain unchanged?
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Unformatted text preview: 1.Consider the following reaction 2NOCl(g) <-> 2NO(g) + Cl2(g) If, initially [NOCl] = 2.43, all others are zero, and at equilibrium, [NO] = 0.7M, calculate the value of Kc. A. 0.109 B. 0.0346 C. 0.140 D. 0.0571 E. 0.156 1.Explain how each of the following affects the amount of H 2 present in an equilibrium mixture in the reaction 3 Fe(s) + 4H2O(g) ↔ Fe3O4(s) + 4H2(g) ∆H° = -150 kJ a. Raising the temperature of the mixture b. Introducing more H 2 O(g); c. Doubling the volume of the container holding the mixture; d. Adding an appropriate catalyst...
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