Write equilibrium constant expressions for the following reactions. For gases, use either pressures or concentrations. (a) 2 H 2 O 2 (g) ⇄ 2 H 2 O(g) + O 2 (g) (b) CO(g) + ½ O 2 g ⇄ CO 2 (g) (c) C(s) + CO 2 (g) ⇄ 2 CO(g) (d) NiO(s) + CO(g) ⇄ Ni(s) + CO 2 (g)
Write equilibrium constant expressions for the following reactions. For gases, use either pressures or concentrations.
(a) 2 H2O2(g) ⇄ 2 H2O(g) + O2(g)
(b) CO(g) + ½ O2g ⇄ CO2(g)
(c) C(s) + CO2(g) ⇄ 2 CO(g)
(d) NiO(s) + CO(g) ⇄ Ni(s) + CO2(g)
(a)
Expert Solution
Interpretation Introduction
Interpretation: The equilibrium constant for the given reaction has to be identified.
Concept Introduction: At equilibrium the concentration of the reaction and the product is equated to a constant K, where K is known as the equilibrium
If a reaction is as aA+bB→cC+dD ,
The equilibrium constant K=[C]c[D]d[A]a[B]b
Answer to Problem 1PS
The equilibrium constant for the reaction is given below,
Kc=[H2O]2[O2][H2O2]2Kp=(H2O)2(O2)(H2O2)2
Explanation of Solution
The equilibrium constant for the reaction can be calculated as,
2H2O2(g)⇄2H2O(g)+O2(g)
The product concentrations appear in the numerator and reactant concentrations appear in the denominator. Each concentration should be raised to a power equal to the stoichiometric coefficient in the balanced equation.
The equilibrium constant for the above reaction is given below,
Kc=[H2O]2[O2][H2O2]2Kp=(H2O)2(O2)(H2O2)2
(b)
Expert Solution
Interpretation Introduction
Interpretation: The equilibrium constant for the given reaction has to be identified.
Concept Introduction: At equilibrium the concentration of the reaction and the product is equated to a constant K, where K is known as the equilibrium
If a reaction is as aA+bB→cC+dD ,
The equilibrium constant K=[C]c[D]d[A]a[B]b
Answer to Problem 1PS
The equilibrium constant for the reaction is given below,
Kc=[CO2][CO][O2]1/2Kp=(CO2)(CO)(O2)1/2
Explanation of Solution
The equilibrium constant for the reaction can be calculated as,
CO(g)+1/2O2(g)⇄CO2(g)
The product concentrations appear in the numerator and reactant concentrations appear in the denominator. Each concentration should be raised to a power equal to the stoichiometric coefficient in the balanced equation.
The equilibrium constant for the above reaction is given below,
Kc=[H2O]2[O2][H2O2]2Kp=(H2O)2(O2)(H2O2)2
(c)
Expert Solution
Interpretation Introduction
Interpretation: The equilibrium constant for the given reaction has to be identified.
Concept Introduction: At equilibrium the concentration of the reaction and the product is equated to a constant K, where K is known as the equilibrium
If a reaction is as aA+bB→cC+dD ,
The equilibrium constant K=[C]c[D]d[A]a[B]b
Answer to Problem 1PS
The equilibrium constant for the reaction is given below,
Kc=[CO]2[C][CO2]Kp=(CO)2(C)(CO2)
Explanation of Solution
The equilibrium constant for the reaction can be calculated as,
C(s)+CO2(g)⇄2CO(g)
The product concentrations appear in the numerator and reactant concentrations appear in the denominator. Each concentration should be raised to a power equal to the stoichiometric coefficient in the balanced equation.
The equilibrium constant for the above reaction is given below,
Kc=[CO]2[C][CO2]Kp=(CO)2(C)(CO2)
(d)
Expert Solution
Interpretation Introduction
Interpretation: The equilibrium constant for the given reaction has to be identified.
Concept Introduction: At equilibrium the concentration of the reaction and the product is equated to a constant K, where K is known as the equilibrium
If a reaction is as aA+bB→cC+dD ,
The equilibrium constant K=[C]c[D]d[A]a[B]b
Answer to Problem 1PS
The equilibrium constant for the reaction is given below,
Kc=[Ni][CO2][NiO][CO]Kp=(Ni)(CO2)(NiO)(CO)
Explanation of Solution
The equilibrium constant for the reaction can be calculated as,
NiC(s)+CO(g)⇄Ni(s)+CO2(g)
The product concentrations appear in the numerator and reactant concentrations appear in the denominator. Each concentration should be raised to a power equal to the stoichiometric coefficient in the balanced equation.
The equilibrium constant for the above reaction is given below,
Kc=[Ni][CO2][NiO][CO]Kp=(Ni)(CO2)(NiO)(CO)
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