- #1
joejo
- 150
- 0
Hi guys can you please check if this is right...thanks in advance
Given the reaction CO2(g) + H2(g) = H2O(g) + CO(g). If initially there are 2.0 moles of CO2 (g) and 2.0 moles of H2(g) introduced into an empty 1.0L container, at 1800ºC, it is found that at equilibrium there are 0.3 moles of CO2 still present. Calculate the Ke value for this reaction at 1800ºC.
CO2(g) + H2(g) = H2O(g) + CO(g)
Initially 2 2 0 0
Equilibrium 2-1.7=.3 2-1.7=.3 1.7 1.7
Ke = 1.7 * 1.7/(.3 * .3) = 32.11
Given the reaction CO2(g) + H2(g) = H2O(g) + CO(g). If initially there are 2.0 moles of CO2 (g) and 2.0 moles of H2(g) introduced into an empty 1.0L container, at 1800ºC, it is found that at equilibrium there are 0.3 moles of CO2 still present. Calculate the Ke value for this reaction at 1800ºC.
CO2(g) + H2(g) = H2O(g) + CO(g)
Initially 2 2 0 0
Equilibrium 2-1.7=.3 2-1.7=.3 1.7 1.7
Ke = 1.7 * 1.7/(.3 * .3) = 32.11