For the reaction 2H2O(g) ⇌ 2H2(g) + O2(g) K = 2.4 × 10-3 at a given temperature. At equilibrium in a 2.0- L container, it is found that [H2O(g)] = 1.1 × 10-1 M and [H2(g)] = 1.9 × 10-2 M. Calculate the moles of O2(g) present under these conditions.
Answer to relevant QuestionsThe reaction 2NO(g) + Br2(g) ⇌ 2NOBr(g) as Kp = 109 at 25oC. If the equilibrium partial pressure of Br2 is 0.0159 atm and the equilibrium partial pressure of NOBr is 0.0768 atm, calculate the partial pressure of NO at ...At a particular temperature, 12.0 moles of SO3 is placed into a 3.0- L rigid container, and the SO3 dissociates by the reaction 2SO3(g) ⇌ 2SO2(g) + O2(g) At equilibrium, 3.0 moles of SO2 is present. Calculate K for this ...For the reaction below at a certain temperature, it is found that the equilibrium concentrations in a 5.00-L rigid container are [H2] = 0.0500 M, [F2] = 0.0100 M, and [HF] = 0.400 M. H2(g) + F2(g) ⇌ 2HF(g) If 0.200 mole of ...At 25oC, Kp = 2.9 × 10-3 for the reaction NH4OCONH2(s) ⇌ 2NH3(g) + CO2(g) In an experiment carried out at 25oC, a certain amount of NH4OCONH2 is placed in an evacuated rigid container and allowed to come to equilibrium. ...An important reaction in the commercial production of hydrogen is CO(g) + H2O(g) ⇌ H2(g) + CO2(g) How will this system at equilibrium shift in each of the five following cases? a. Gaseous carbon dioxide is removed. b. ...
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