Kp and Kc

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.