At a certain temperature, 0.350 mol CH, and 0.676 mol H, S are placed in a 2.50 L container. CH,(g) + 2 H, S(g) = CS,(g) + 4 H, (g) At equilibrium, 10.4 g CS, is present. Calculate Ke. 57 K. = Incorrect

3.6

While ethanol CH3CH2OH is produced naturally by fermentation, e.g. in beer- and wine-making, industrially it is synthesized by reacting ethylene CH2CH2 with water vapor at elevated temperatures. A chemical engineer studying this reaction fills a 75L tank with 16.mol of ethylene gas and 27.mol of water vapor. When the mixture has come to equilibrium she determines that it contains 9.6mol of ethylene gas and 20.6mol of water vapor. The engineer then adds another 9.0mol of water, and allows the mixture to come to equilibrium again. Calculate the moles of ethanol after equilibrium is reached the second time. Round your answer to 2 significant digits.

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At a certain temperature, 0.391 mol CH, and 0.768 mol H, S are placed in a 3.00 L container. CH,(g) + 2 H,S(g) = CS,(g) + 4 H,(g) At equilibrium, 11.7 g CS, is present. Calculate K.. Ke & TOOLS x10"

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For the reaction 2CH4 (g) = C2H2(g) + 3H2(g) K. = 0.140 at 1756 °C.What is K, for the reaction at this temperature? %3D Express your answer numerically.

While ethanol (CH3CH,OH) is produced naturally by fermentation, e.g. in beer- and wine-making, industrially it is synthesized by reacting ethylene (CH,CH,) with water vapor at elevated temperatures. A chemical engineer studying this reaction fills a 500. mL flask with 0.77 atm of ethylene gas and 0.98 atm of water vapor. When the mixture has come to equilibrium he determines that it contains 0.34 atm of ethylene gas and 0.55 atm of water vapor. The engineer then adds another 0.19 atm of ethylene, and allows the mixture to come to equilibrium again. Calculate the pressure of ethanol after equilibrium is reached the second time. Round your answer to 2 significant digits. atm

2. According to Le Chatelier's principle, it indicates where the balance is favored (Reactants or products) of the following unbalanced reaction H₂O(a) + Fe(s) + H₂(g) + Fe3O4(s) + Heat Write your answer on the line a) Decreases ia [H2): b) The temperature of the system decreases: c) The system pressure increases:

2 HBr(g) ↔ H2(g) + Br2(g) this reaction has an equilibrium constant Kp = (8.5x10^-5). If the equilibrium partial pressure of H2(g) is (7.22x10^-1) bar and Br2(g) is (4.02x10^0) bar, what the is equilibrium partial pressure of HBr in bar?