1)If the temperature is increased and some oxygen is removed, how does this affect the amount of the Cl2 present at equilibrium for the following reaction? 4 HCl(g) + O2(g) ? 2 H2O(g) + 2 Cl2(g) ?H

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13 Dec 2019

1)If the temperature is increased and some oxygen is removed, how does this affect the amount of the Cl₂ present at equilibrium for the following reaction?
4 HCl(g) + O₂(g) ? 2 H₂O(g) + 2 Cl₂(g) ?H

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Casey DurganLv2

17 Dec 2019

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A mixture of 0.02471 mol of Cl2, 0.02489 mol of H2O, 0.06124 mol of HCl, and 0.03210 mol of O2 is placed in a 1.0-L steel pressure vessel at 1977 K. The following equilibrium is established:2 Cl2(g) + 2 H2O(g) 4 HCl(g) + 1 O2(g)At equilibrium 0.01509 mol of Cl2 is found in the reaction mixture.(a) Calculate the equilibrium partial pressures of Cl2, H2O, HCl, and O2.Peq(Cl2) = .Peq(H2O) = .Peq(HCl) = .Peq(O2) = .(b) Calculate KP for this reaction.KP = .

Consider the following equilibrium, for which K_p = 0.0752 at 480 °C:

2 Cl₂(g) + 2 H₂O(g) 4 HCl(g) + O₂(g)

(a) What is the value of K_p for the reaction 4 HCl(g) + O₂(g) 2 Cl₂(g) + 2 H₂O(g)? (b) What is the value of K_p for the reaction Cl₂(g) + H₂O(g) 2 HCl(g) + O₂(g)? (c) What is the value of K_c for the reaction in part (b)?