Question

In: Chemistry

Consider the reaction CO(g) + 3 H2 (g) ⇌ CH4 (g) + H2O(g) Kc = 7.7×10–23...

Consider the reaction CO(g) + 3 H2 (g) ⇌ CH4 (g) + H2O(g) Kc = 7.7×10–23 at 25 °C. 1.50 mol CH4 and 2.50 mol H2O are added to an empty 2.00-L container at 25 °C and allowed to reach equilibrium. What are the equilibrium amounts (in moles) of each species?

The answer is: 1.5 mol CO, 4.5 mol H2 , 1.0 mol H2O, and 2.6×10–21 mol CH4. Please include written work and explanation :-) Thank you!

Solutions

Expert Solution


Related Solutions

Consider the reaction CO(g) + 3 H2 (g) ⇌ CH4 (g) + H2O(g) Kc = 7.7×10–23...
Consider the reaction CO(g) + 3 H2 (g) ⇌ CH4 (g) + H2O(g) Kc = 7.7×10–23 at 25 °C. 1.50 mol CH4 and 2.50 mol H2O are added to an empty 2.00-L container at 25 °C and allowed to reach equilibrium. What are the equilibrium amounts (in moles) of each species? The answer is: 1.5 mol CO, 4.5 mol H2 , 1.0 mol H2O, and 2.6×10–21 mol CH4. Please include written work and explanation :-) Thank you!
For the equilibrium system CO (g) + 3 H2 (g) ⇌ H2O (g) + CH4 (g),...
For the equilibrium system CO (g) + 3 H2 (g) ⇌ H2O (g) + CH4 (g), ΔH = -206 kJ/mol, state whether the yield of CH4 will increase, decrease or remain the same for the following changes: Adding some H2 gas to the system Removing H2O from the system Increasing the volume of the system Decreasing the temperature on the system Adding a catalyst to the system
Consider the reaction: CO(g)+H2O(g)⇌CO2(g)+H2(g) Kc=102 at 500 K A reaction mixture initially contains 0.135 M CO...
Consider the reaction: CO(g)+H2O(g)⇌CO2(g)+H2(g) Kc=102 at 500 K A reaction mixture initially contains 0.135 M CO and 0.135 M H2O. What is the equilibrium concentration of [CO], [H2O], [CO2], and [H2]
Consider the following reaction: CO (g) + H2O (g) ⇌ CO2 (g) + H2(g) If you...
Consider the following reaction: CO (g) + H2O (g) ⇌ CO2 (g) + H2(g) If you start with a mixture containing 1.00 mol of CO and 1.00 mol of H2O, calculate the number of moles of each component in the mixture when equilibrium is reached at 1000 °C. The mixture contains 0.43 mol H2? nCO = nH2O = nCO2 = How do I work this out?
Consider the reaction: CO(g) + H2O(g)<------> CO(g) + H2(g)   and K = 0.118 at 4000 K....
Consider the reaction: CO(g) + H2O(g)<------> CO(g) + H2(g)   and K = 0.118 at 4000 K. A reaction mixture initially contains a CO partial pressure of 1344 mbar and a H2O partial pressure of 1766 mbar at 4000K. Calculate the equilibrium partial pressures of each of the products.
Consider the following equilibrium: CO2(g) + H2(g)---CO(g) + H2O(g); Kc = 1.6 at 1260 K Suppose...
Consider the following equilibrium: CO2(g) + H2(g)---CO(g) + H2O(g); Kc = 1.6 at 1260 K Suppose 0.038 mol CO2 and 0.022 mol H2 are placed in a 1.50-L vessel at 1260 K. What is the equilibrium partial pressure of CO(g)? The answer is either 9.9 atm or 1.1 atm. But my question is WHY IS ONE CHOICE INCORRECT since I get both in my calculations.
Consider the following chemical reaction: 2 CH4(g) 3 O2(g) 2 CO(g) 4 H2O(l) Select all the...
Consider the following chemical reaction: 2 CH4(g) 3 O2(g) 2 CO(g) 4 H2O(l) Select all the statements that are correct: The reaction should become more product favored at high temperatures The reaction should become more product favored at low temperatures The reactants can adopt a larger number of configurations than the products The potential energy of the reactants is higher than the potential energy of the products The potential energy of the reactants is lower than the potential energy of...
23.Consider the following equilibrium process at 686°C: CO2(g) + H2(g) ⇌ CO(g) + H2O(g) The equilibrium...
23.Consider the following equilibrium process at 686°C: CO2(g) + H2(g) ⇌ CO(g) + H2O(g) The equilibrium concentrations of the reacting species are [CO] = 0.0580 M, [H2] = 0.0430 M, [CO2] = 0.0900 M, and [H2O] = 0.0420 M. (a) Calculate Kc for the reaction at 686°C. ________ (b) If we add CO2 to increase its concentration to 0.460 mol / L, what will the concentrations of all the gases be when equilibrium is reestablished? CO2: M H2: M CO:...
Consider the following reaction: CO(g)+H2O(g)⇌CO2(g)+H2(g) Kp=0.0611 at 2000 K A reaction mixture initially contains a CO...
Consider the following reaction: CO(g)+H2O(g)⇌CO2(g)+H2(g) Kp=0.0611 at 2000 K A reaction mixture initially contains a CO partial pressure of 1336 torr and a H2O partial pressure of 1764 torr at 2000 K. Part A Calculate the equilibrium partial pressure of CO2. Part B Calculate the equilibrium partial pressure of H2.
Consider the reaction: CO(g)+H2O(g)⇌CO2(g)+H2(g) K=0.118 at 4000 K A reaction mixture initially contains a CO partial...
Consider the reaction: CO(g)+H2O(g)⇌CO2(g)+H2(g) K=0.118 at 4000 K A reaction mixture initially contains a CO partial pressure of 1361 mbar and a H2O partial pressure of 1781 mbar at 4000 K. Part A: Calculate the equilibrium partial pressure of CO in bar using three decimal places Part B: Calculate the equilibrium partial pressure of H2O in bar using three decimal places. Part C: Calculate the equilibrium partial pressure of CO2 in bar using three decimal places Part D: Calculate the...
ADVERTISEMENT
ADVERTISEMENT
ADVERTISEMENT