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# 8 - just calculated and make a prediction ∆n = Number of...

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17.35 To decide if the reaction is at equilibrium, calculate Qp and compare it to Kp. If Qp = Kp, then the reaction is at equilibrium. If Qp > Kp, then the reaction proceeds to the left to produce more reactants. If Qp < Kp, then the reaction proceeds to the right to produce more products. Qp > Kp, thus, the reaction is not at equilibrium and will proceed to the left (towards the reactants). 17.36 Qp = Qp < Kp Thus, the reaction is not at equilibrium and will proceed to the right (towards the products). 17.37 There is insufficient information to calculate the partial pressures of each gas (T is not given). There is sufficient information to determine the concentrations and hence Qc . Convert the Kp given to Kc using Kp = Kc Compare the Qc to the Kc
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Unformatted text preview: just calculated and make a prediction. ∆n = Number of product gas moles - Number of reactant gas moles = 2 - 2 = 0 Since ∆n = 0, Kp = Kc = 2.7 (note if ∆n had any other value, we could not finish the calculation without the temperature.) Thus, the reaction is not at equilibrium and will proceed to the left (towards the reactants). 17.38 At equilibrium, equal concentrations of CFCl3 and HCl exist, regardless of starting reactant concentrations. The equilibrium concentrations of CFCl3 and HCl would still be equal if unequal concentrations of CCl4 and HF were used. This occurs only when the two products have the same coefficients in the balanced equation. Otherwise, more of the product with the larger coefficient will be produced....
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