1-At 1130°C, the equilibrium constant (Kc) for the reaction 2H2S(g) â 2H2(g) + S2(g) is 2.25 à 10â4. If [H2S] = 4.70 à 10â3 M and [H2] = 1.50 à 10â3 M, calculate [S2] ? M (Enter your answer in scientific notation.)
2-The equilibrium constant Kc for the reaction H2(g) + CO2(g) â H2O(g) + CO(g) is 4.2 at 1650°C. Initially 0.86 mol H2 and 0.86 mol CO2 are injected into a 4.8âL flask. Calculate the concentration of each species at equilibrium.
Equilibrium concentration of H2:?M
Equilibrium concentration of CO2:? M
3-The equilibrium constant Kc for the equation 2H2(g) + CO(g) â CH3OH(g) is 11 at a certain temperature. If there are 2.63Ã10â2 moles of H2 and 7.15 Ã10â3 moles of CH3OH at equilibrium in a 6.29âL flask, what is the concentration of CO?
1-At 1130°C, the equilibrium constant (Kc) for the reaction 2H2S(g) â 2H2(g) + S2(g) is 2.25 à 10â4. If [H2S] = 4.70 à 10â3 M and [H2] = 1.50 à 10â3 M, calculate [S2] ? M (Enter your answer in scientific notation.)
2-The equilibrium constant Kc for the reaction H2(g) + CO2(g) â H2O(g) + CO(g) is 4.2 at 1650°C. Initially 0.86 mol H2 and 0.86 mol CO2 are injected into a 4.8âL flask. Calculate the concentration of each species at equilibrium.
Equilibrium concentration of H2:?M
Equilibrium concentration of CO2:? M
3-The equilibrium constant Kc for the equation 2H2(g) + CO(g) â CH3OH(g) is 11 at a certain temperature. If there are 2.63Ã10â2 moles of H2 and 7.15 Ã10â3 moles of CH3OH at equilibrium in a 6.29âL flask, what is the concentration of CO?