Multiple Choice
The Keq for the equilibrium below is 5.4 x 10^13 at 480.0°C.
2NO (g) + O2 (g) ↔ 2NO2 (g)
What is the value of Keq at this temperature for the following reaction?
NO (g) + 1/2 O2 (g) ↔ NO2 (g)
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16. Chemical Equilibrium
Equilibrium Constant K
Multiple Choice
What is the equilibrium chemical equation for a 0.01 M solution of sodium acetate, NaC2H3O2(aq)?
A
NaC2H3O2(aq) ⇌ NaC2H3O2(g)
B
NaC2H3O2(aq) ⇌ Na+(aq) + C2H3O2−(aq)
C
NaC2H3O2(aq) ⇌ NaC2H3O2(s)
D
NaC2H3O2(aq) ⇌ Na2C2H3O2(aq)
Verified step by step guidance1
Identify the nature of sodium acetate (NaC2H3O2) in an aqueous solution. Sodium acetate is a salt that can dissociate into its constituent ions in water.
Recognize that in an aqueous solution, sodium acetate will dissociate into sodium ions (Na+) and acetate ions (C2H3O2−). This is a common behavior for ionic compounds in water.
Write the dissociation equation for sodium acetate in water: NaC2H3O2(aq) ⇌ Na+(aq) + C2H3O2−(aq). This represents the equilibrium between the undissociated salt and its ions in solution.
Understand that the other options provided involve incorrect states or products for sodium acetate in an aqueous solution. For example, NaC2H3O2(g) suggests a gaseous state, which is not applicable here, and Na2C2H3O2(aq) suggests a different compound.
Conclude that the correct equilibrium chemical equation for a 0.01 M solution of sodium acetate is NaC2H3O2(aq) ⇌ Na+(aq) + C2H3O2−(aq), as it accurately represents the dissociation of the salt into its ions in water.
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