Kp and Kc

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Table of Contents: • 00:34 - Kp and Kc • 00:35 - Equilibrium Constant Expressions • 01:47 - Pressure Equilibrium Constant Expression • 02:33 - 2 H2O(g) ⇄ 2 H2(g) + O2(g) • 03:58 - 2 HF(g) ⇄ H2(g) + F2(g) • 05:08 - Relationship Between Kp and Kc • 06:01 - 1. Ammonia decomposes upon heating by the following reaction 2 NH3(g) ⇄ 3 H2(g) + N2(g).a. If Kc = 9.31 x 10-3 at 800°C, what is Kp at this temperature?b. If a 2.50 L vessel contained 0.0185 mol of ammonia (NH3), 0.158 mol of hydrogen gas, and 0.870 mol nitrogen gas at 298 K in an equilibrium mixture. Calculate the value of Kc at 298 K.c. Calculate the value of Kp at 298 K. • 06:54 - 1. Ammonia decomposes upon heating by the following reaction 2 NH3(g) ⇄ 3 H2(g) + N2(g). • a. If Kc = 9.31 x 10-3 at 800°C, what is Kp at this temperature? • 08:07 - 1. Ammonia decomposes upon heating by the following reaction 2 NH3(g) ⇄ 3 H2(g) + N2(g). • b. If a 2.50 L vessel contained 0.0185 mol of ammonia (NH3), 0.158 mol of hydrogen gas, and 0.870 mol nitrogen gas at 298 K in an equilibrium mixture. Calculate the value of Kc at 298 K. • 09:11 - 1. Ammonia decomposes upon heating by the following reaction 2 NH3(g) ⇄ 3 H2(g) + N2(g). • c. Calculate the value of Kp at 298 K. • 09:45 - 2. Consider the following reaction at 1000°C: • CO(g) + 3H2(g) ⇄ CH4(g) + H2O(g). At equilibrium, the following pressures are measured: pCO = 0.0613 atm, pH2 = 0.1839 atm, pCH4 = 0.0387 atm, and pH2O = 0.0387 atm. Calculate the value of Kp for this reaction. Calculate the value of Kc.

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