(a)
Interpretation:
Whether the following reaction is in equilibrium or not has to be determined.
Concept Introduction:
The condition of equilibrium is a state of balance of processes that runs in opposite directions. At equilibrium, the formation of a product from the reactant balances the formation of reactant from the product. Also, the change in concentration of reaction and product seems to be negligible at the equilibrium state.
A reaction quotient
The general equilibrium reaction is as follows:
Here,
The expression of the reaction quotient for the above reaction is as follows:
Here,
The concentration of reactants and products changes in order to bring reaction quotient and equilibrium constant closer. Therefore, the direction of reaction can be predicted as follows:
(1) If
(2)If
(3)If
(b)
Interpretation:
If the following reaction is not at equilibrium then the direction of reaction has to be determined.
Concept Introduction:
Refer to part (a).
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Chapter 14 Solutions
Chemistry: Principles and Practice
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- For the reaction N2(g)+3H2(g)2NH3(g) show that Kc = Kp(RT)2 Do not use the formula Kp = Kc(RT)5n given in the text. Start from the fact that Pi = [i]RT, where Pi is the partial pressure of substance i and [i] is its molar concentration. Substitute into Kc.arrow_forwardA solution is prepared by dissolving 0.050 mol of diiodocyclohexane, C5H10I2, in the solvent CCl4.The total solution volume is 1.00 L When the reaction C6H10I2 C6H10 + I2 has come to equilibrium at 35 C, the concentration of I2 is 0.035 mol/L. (a) What are the concentrations of C6H10I2 and C6H10 at equilibrium? (b) Calculate Kc, the equilibrium constant.arrow_forwardSuppose a reaction has the equilibrium constant K = 1.3 108. What does the magnitude of this constant tell you about the relative concentrations of products and reactants that will be present once equilibrium is reached? Is this reaction likely to be a good source of the products?arrow_forward
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