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Ch.15 - Chemical Equilibrium
Tro - Chemistry: A Molecular Approach 4th Edition
Tro4th EditionChemistry: A Molecular ApproachISBN: 9780134112831Non è quello che usi tu?Cambia libro di testo
Tutti i libri di testoTro 4th EditionCh.15 - Chemical EquilibriumProblema 31b,c
Capitolo 15, Problema 31b,c

Calculate Kc for each reaction.
b. CH4(g) + H2O(g) ⇌ CO(g) + 3 H2(g) Kp = 7.7x1024 (at 298 K)
c. I2(g) + Cl2(g) ⇌ 2 ICl(g) Kp = 81.9 (at 298 K)

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1
Identify the relationship between Kc and Kp using the equation: Kc = Kp(RT)^-Δn, where R is the ideal gas constant (0.0821 L·atm/mol·K) and T is the temperature in Kelvin.
Determine Δn, the change in moles of gas, by subtracting the sum of the moles of gaseous reactants from the sum of the moles of gaseous products. For the given reaction, Δn = (1 + 3) - (1 + 1).
Substitute the given values into the equation: Kc = 7.7x10^24 * (0.0821 * 298)^-Δn.
Calculate the value of (RT)^-Δn using the values of R, T, and Δn.
Multiply Kp by the calculated value of (RT)^-Δn to find Kc.

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Equilibrium Constant (Kc and Kp)

The equilibrium constant (K) quantifies the ratio of the concentrations of products to reactants at equilibrium for a given reaction. Kc refers to concentrations in molarity, while Kp refers to partial pressures. The relationship between Kc and Kp is given by the equation Kp = Kc(RT)^(Δn), where Δn is the change in moles of gas. Understanding this relationship is crucial for converting between Kc and Kp.
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Kp vs. Kc Formula

Reaction Quotient (Q)

The reaction quotient (Q) is a measure of the relative amounts of products and reactants at any point in a reaction, not just at equilibrium. It is calculated using the same formula as K, but with the current concentrations or pressures. Comparing Q to K helps predict the direction in which a reaction will proceed to reach equilibrium, which is essential for understanding dynamic chemical systems.
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Reaction Quotient Q

Le Chatelier's Principle

Le Chatelier's Principle states that if a system at equilibrium is disturbed by changes in concentration, temperature, or pressure, the system will adjust to counteract the disturbance and restore a new equilibrium. This principle is vital for predicting how changes in conditions will affect the position of equilibrium and the values of Kc and Kp in a given reaction.
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Le Chatelier's Principle
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