Starting with 0.100 mol each of CO(g) and H2O(g) in a 5.00 L flask at 600 K;
CO(g) + H2O(g) CO2(g) + H2 (g) Kc = 23.2 at 600 K
Starting with 0.100 mol each of CO(g) and H2O(g) in a 5.00 L flask at 600...
The equilibrium constant Kc for the reaction H2(g) + CO2(g) ⇌ H2O(g) + CO(g) is 4.2 at 1650°C. Initially 0.71 mol H2 and 0.71 mol CO2 are injected into a 5.0−L flask. Calculate the concentration of each species at equilibrium.
A mixture of 3.00 mol of Cl2 and 3.00 mol of CO is enclosed in a 5.00-L flask at 600.°C. At equilibrium, 3.3% of the Cl2 has been consumed. CO(g) + Cl2(g) = COCl2(g) Calculate Kc for the reaction at 600.°C. Calculate deltaG for the reaction at this temperature. = kJ/mol CO(g)= deltaH= -110.5 (kJ/mol) deltaG= -137.2 (kj/mol) S= 197.7 (j/molK) Cl2(g)= S= 223.1 J/molK COCl2(g)= deltaH= -218.8(kJ/mol) deltaG= -204.6 (kj/mol) S= 197.7 J/molK
4. Consider the following reaction at equilibrium CO(g) + H2O(g) + CO2(g) + H2(g) 2.50 mole of CO(g) and 2.50 mole of H2O(g) gas at 588 K are mixed in a 10.00 L container. (Kc = 31.4 at 588 K) Calculate the concentration of CO(g), H2O(g), CO (g), and H.(g) at equilibrium. 5. Consider the following reaction: CO(g) + H2O(g) + CO2(g) + H2(g) (a) If a 10.00L container has 2.50 mole of CO(g), 2.50 mole of H2O(g), 5.00 mole...
Be sure to answer all parts. The equilibrium constant K, for the reaction Hz() + CO2() H2O(g) + CO(g) 1s 4.2 at 1650°C. Initially 0.76 mol H2 and 0.76 mol CO2 are injected into a 4.5-L flask. Calculate the concentration of each species at equilibrium. Equilibrium concentration of H2: Equilibrium concentration of CO2: Equilibrium concentration of H20: Equilibrium concentration of CO:
Let's work a more challenging problem..... 1.00 g of each CO, H2O, and H, are sealed in a 1.41 L vessel and brought to equilibrium at 600 K. How many grams of Co, will be present in the equilibrium mixture? (K = 23.2) CO(g) + H2O(g) + CO2(g) + H2(g)
Be sure to answer all parts. The equilibrium constant Kc for the reaction H2(g) + CO2(g) ⇌ H2O(g) + CO(g) is 4.2 at 1650°C. Initially 0.72 mol H2 and 0.72 mol CO2 are injected into a 4.5−L flask. Calculate the concentration of each species at equilibrium. Equilibrium concentration of H2: M Equilibrium concentration of CO2: M Equilibrium concentration of H2O: M Equilibrium concentration of CO: M
The equilibrium constant Kc for the following reaction is 8.30. H2(g) + CO2(g) ↔ H2O(g) + CO(g) Initially, 0.40 moles each of H2 and CO2 are injected into a 9.00 L flask. Calculate the concentration of the CO(g) at equilibrium.
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] = 0.0480 M, [H2] = 0.0400 M, [CO2] = 0.0880 M, and [H2O] = 0.0430 M. (a) Calculate Kc for the reaction at 686 ° C. (b) If we add CO2 to increase its concentration to 0.510 mol / L, what will the concentrations of all the gases be when equilibrium is reestablished? CO2: M...
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] = 0.0830 M, and [H2O] = 0.0370 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: M...
5-7 (ACS-style) A mixture of 2.0 mol of CO (g) and 2.0 mol of H20 (g) was allowed to come to equilibrium in a 10.0-L flask at a high temperature. If Kc = 4.0, what is the molar concentration of H2 (g) in the equilibrium mixture? The equation for the reaction is: CO(g) + H20 (g) 5 CO2(g) + H2 (g) A) 0.67 M B) 0.40 M C) 0.20 M D) 0.13 M