Exam3DKey

Exam3DKey - 1) (25) At some temperature, K = 0.138 for the...

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1) (25) At some temperature, K = 0.138 for the following reaction: H 2 O(g) + CO(g) ¾ H 2 (g) + CO 2 (g) The initial partial pressures of H 2 O and CO are each 0.750 atm. The system is then allowed to equilibrate. What is the equilibrium pressure of CO? H 2 O(g) + CO(g) ¾ H 2 (g) + CO 2 (g) i 0.750 0.750 0 0 atm -x -x +x +x atm e 0.750 – x 0.750 – x x x atm K = P(CO) O) P(H ) P(CO ) P(H 2 2 2 0.138 = x) - (0.750 x) - (0.750 (x) (x) 0.371 = x - 0.750 x 0.279 – 0.371 x = x 0.279 = 1.371 x 0.202 = x P(CO 2 ) = 0.750 – 0.203 = 0.547 atm 2) (25) At some temperature, 2.00 moles of NH 3 are placed in a 1.00 L container and allowed to equilibrate according to the equation: 2 NH 3 ¾ N 2 + 3 H 2 At equilibrium, 0.72 moles of NH 3 remain. What is the value of K c for this reaction? 2 NH 3 ¾ N 2 + 3 H 2 i 2.00 0 0 M -1.28 +0.64 + 1.92 M e 0.72 0.64 1.92 M K c = 2 3 3 2 2 ] [NH ] [H ] [N = 2 3 (0.72) (1.92) (0.64) = K c = 8.7
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3) A solution is labeled 0.150 M NH 3 (aq). a) (25) What is the concentration of NH
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Exam3DKey - 1) (25) At some temperature, K = 0.138 for the...

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