Given that Kc = 1.6×10?34 at 25 °C for this reaction: 2 HCl(g) + I2(s) ? 2 HI(g) + Cl2(g) a. What is Kp at 25 °C for the same reaction? Determine the value of Kc for each of the following reactions:...

Given that Kc = 1.6×10?34 at 25 °C for this reaction: 2 HCl(g) + I2(s) ? 2 HI(g) + Cl2(g) a. What is Kp at 25 °C for the same reaction? Determine the value of Kc for each of the following reactions: b. 2 HI(g) + Cl2(g) ? 2 HCl(g) + I2(s) c. 4 HCl(g) + 2 I2(s) ? 3 HI(g) + 2 Cl2(g) d. HI(g) + ½ Cl2(g) ? HCl(g) + ½ I2(s XXXXXXXXXXFind Kp for this reaction: N2O(g) + NO2(g) ? 3 NO(g) Given: N2(g) + O2(g) ? 2 NO(g) Kp = 2.3×10?3 2 NO(g) + O2(g) ? 2 NO2(g) Kp = 7.4×10?6 2 N2O(g) ? 2 N2(g) + O2(g) Kp = 1.9× XXXXXXXXXXConsider the following system at equilibrium: 2 PbS(s) + 3 O2(g) ? 2 PbO(s) + 2 SO2(g) ?H° = XXXXXXXXXXkJ For each of the following changes … (1) Would the equilibrium yield of PbO increase, decrease, or remain unchanged? Explain. (2) Would the value of the equilibrium constant increase, decrease, or remain unchanged? Explain. a. increasing PO2 d. increasing the volume b. adding SO2 to the system e. increasing the total pressure by adding argon c. decreasing the temperature f. adding a catalyst 15-4. When carbon monoxide reacts with hydrogen gas, methane and steam are formed: CO(g) + 3 H2 (g) ? CH4 (g) + H2O(g) At 1127 °C, analysis at equilibrium shows the presence of XXXXXXXXXXmol CO, XXXXXXXXXXmol H2, XXXXXXXXXXmol CH4 and XXXXXXXXXXmol H2O in a 4.00 liter container. a. Calculate Kc for this reaction at 1127 °C. b. Calculate Kp for this reaction at 1127 °C XXXXXXXXXXConsider the reaction between ammonia and oxygen: 4 NH3 (g) + 3 O2 (g) ? 2 N2 (g) + 6 H2O(g) At a certain temperature, Kp = XXXXXXXXXXCalculate the equilibrium partial pressure of ammonia if (PN2 )E = 0.213 atm, (PH2O )E = 0.883 atm and (PO2 )E = 0.255 atm XXXXXXXXXXDetermine the equilibrium constant for this reaction: 2 NO2Cl(g) ? Cl2(g) + 2 NO2(g) The container is initially charged with XXXXXXXXXXatm of NO2Cl and XXXXXXXXXXatm of Cl2, and at equilibrium, the pressure of NO2 is XXXXXXXXXXatm XXXXXXXXXXPure hydrogen cyanide, at 0.120 M is placed into a sealed vessel and heated to 375 K. When the system reaches equilibrium, it is found that 33.0% of the hydrogen cyanide has decomposed to cyanogen (C2N2) and hydrogen: 2 HCN(g) ? C2N2 (g) + H2 (g) Calculate Kc for this reaction at 375 K XXXXXXXXXXAt 100 °C, Kc = XXXXXXXXXXfor this reaction: SO2Cl2(g) ? SO2(g) + Cl2(g) Suppose initially [SO2Cl2] = XXXXXXXXXXM, [SO2] = XXXXXXXXXXM, and [Cl2] = XXXXXXXXXXM. a. Will the reaction go left or right to reach equilibrium? b. What are the equilibrium concentrations of all species? 15-9. At 150 °C, Kc = XXXXXXXXXXfor this reaction: 2 IBr(g) ? I2 (g) + Br2 (g) Pure IBr is placed into a 4.00 L vessel. At equilibrium, the concentration of Br2 is XXXXXXXXXXM. How many grams of IBr were initially put into the vessel?