A sample of S8(g) is placed in an otherwise empty, rigid container at 1325 K at an initial pressure of 1.00 atm, where it decomposes to S2(g) by the reaction S8(g) ⇌ 4S2(g) At equilibrium, the partial pressure of S8 is 0.25 atm. Calculate Kp for this reaction at 1325 K.
Answer to relevant QuestionsAt 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 ...At a particular temperature, K = 3.75 for the reaction SO2(g) + NO2(g) ⇌ SO3(g) + NO(g) If all four gases had initial concentrations of 0.800 M, calculate the equilibrium concentrations of the gases. At a particular temperature, K = 2.0 × 10-6 for the reaction 2CO2(g) ⇌ 2CO(g) + O2(g) If 2.0 moles of CO2 is initially placed into a 5.0-L vessel, calculate the equilibrium concentrations of all species. Suppose the reaction system UO2(s) + 4HF(g) ⇌ UF4(g) + 2H2O(g) has already reached equilibrium. Predict the effect that each of the following changes will have on the equilibrium position. Tell whether the equilibrium will ...Given the following equilibrium constants at 427oC, Na2O(s) ⇌ 2Na(l) + 12 O2(g) K1 = 2 × 10-25 NaO(g) ⇌ Na(l) + l2 O2(g) K2 = 2 × 10-5 Na2O2(s) ⇌ 2Na(l) + O2(g) K3 = 5 × 10-29 NaO2(s) ⇌ Na(l) + O2(g) K4 = 3 × ...
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