Multiple Choice
A solution initially contains [Ag+] of 3.2 × 10^-3 M and 0.125 M NH3. What is the concentration of Ag+ after the solution reaches equilibrium, given that the formation constant (Kf) of Ag(NH3)2+ is 1.7 × 10^7?
16. Chemical Equilibrium
Equilibrium Constant Calculations
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Calculate the equilibrium constant (K) for the reaction: 2 N2O (g) + 3 O2 (g) ⇌ 2 N2O4 (g), using the following information: 1) 2 N2 (g) + O2 (g) ⇌ 2 N2O (g) K1 = 1.2 x 10^-35 2) N2O4 (g) ⇌ 2 NO2 (g) K2 = 4.6 x 10^-3 3) ½ N2 (g) + O2 (g) ⇌ NO2 (g) K3 = 4.1 x 10^-9
A
K = 4.9 x 10^5
B
K = 2.5 x 10^-31
C
K = 1.3 x 10^31
D
K = 3.8 x 10^-5
Verified step by step guidance1
Identify the target reaction: 2 N2O (g) + 3 O2 (g) ⇌ 2 N2O4 (g). We need to find the equilibrium constant (K) for this reaction using the given reactions and their equilibrium constants.
Recognize that the given reactions can be manipulated to form the target reaction. The first reaction, 2 N2 (g) + O2 (g) ⇌ 2 N2O (g), can be reversed to form N2O from N2 and O2. The equilibrium constant for the reverse reaction is the reciprocal of K1.
The second reaction, N2O4 (g) ⇌ 2 NO2 (g), can be reversed to form N2O4 from NO2. The equilibrium constant for the reverse reaction is the reciprocal of K2.
The third reaction, ½ N2 (g) + O2 (g) ⇌ NO2 (g), can be used directly. However, it needs to be multiplied by 2 to match the stoichiometry of the target reaction. The equilibrium constant for this adjusted reaction is K3 squared.
Combine the manipulated reactions to form the target reaction. Multiply the equilibrium constants of the manipulated reactions to find the equilibrium constant for the target reaction. This involves multiplying the reciprocal of K1, the reciprocal of K2, and K3 squared.
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