(a)
Interpretation:
The equilibrium constant expression for Kp and the equation that relates Kp and Kc for the equation
Concept introduction:
Equilibrium constant expression for gas-phase reactions are written using partial pressures.
PA, PB and PC are partial pressures of A, B and C gases respectively.
The concentration or partial pressure of pure solids and pure liquids are not included in the equilibrium constant expression.
The relationship between Kp and Kc is given by the following equation.
Kp = equilibrium constant in terms of partial pressure
Kc = equilibrium constant in terms of concentrations.
R = universal gas constant
T = absolute temperature
(b)
Interpretation:
The equilibrium constant expression for Kp and the equation that relates Kp and Kc for the equation
Concept introduction:
Equilibrium constant expression for gas-phase reactions are written using partial pressures.
PA, PB and PC are partial pressures of A, B and C gases respectively.
The concentration or partial pressure of pure solids and pure liquids are not included in the equilibrium constant expression.
The relationship between Kp and Kc is given by the following equation.
Kp = equilibrium constant in terms of partial pressure
Kc = equilibrium constant in terms of concentrations.
R = universal gas constant
T = absolute temperature
(c)
Interpretation:
The equilibrium constant expression for Kp and the equation that relates Kp and Kc for the equation
Concept introduction:
Equilibrium constant expression for gas-phase reactions are written using partial pressures.
PA, PB and PC are partial pressures of A, B and C gases respectively.
The concentration or partial pressure of pure solids and pure liquids are not included in the equilibrium constant expression.
The relationship between Kp and Kc is given by the following equation.
Kp = equilibrium constant in terms of partial pressure
Kc = equilibrium constant in terms of concentrations.
R = universal gas constant
T = absolute temperature
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CHEMISTRY-TEXT
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