Multiple Choice
Given the equilibrium reactions:A(g) + B2(g) <==> AB(g) + B(g) with KC = 4AB(g) <==> A(g) + B(g) with KC = 0.5What is the equilibrium constant (KC) for the following reaction?2A(g) + B2(g) <==> 2AB(g)
16. Chemical Equilibrium
Equilibrium Constant Calculations
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Given that Kc is 1.67 × 10^20 at 25°C for the formation of the iron(III) oxalate complex ion: Fe3+(aq) + 3 C2O4^2-(aq) ⇌ [Fe(C2O4)3]^3-(aq), and 0.0200 M Fe3+ is initially mixed with 1.00 M oxalate ion, what is the concentration of Fe3+ ion at equilibrium?
A
0.50 M
B
1.00 × 10^-22 M
C
0.0200 M
D
0.0100 M
Verified step by step guidance1
Start by writing the expression for the equilibrium constant (Kc) for the reaction: \( K_c = \frac{[Fe(C_2O_4)_3]^{3-}}{[Fe^{3+}][C_2O_4^{2-}]^3} \).
Identify the initial concentrations: \([Fe^{3+}] = 0.0200 \text{ M}\) and \([C_2O_4^{2-}] = 1.00 \text{ M}\). Assume \([Fe(C_2O_4)_3]^{3-}\) is initially 0 M.
Define the change in concentration at equilibrium using the variable \(x\): \([Fe^{3+}] = 0.0200 - x\), \([C_2O_4^{2-}] = 1.00 - 3x\), and \([Fe(C_2O_4)_3]^{3-} = x\).
Substitute these expressions into the Kc equation: \( K_c = \frac{x}{(0.0200 - x)(1.00 - 3x)^3} \).
Solve for \(x\) using the given value of \(K_c = 1.67 \times 10^{20}\), which will allow you to find the equilibrium concentration of \([Fe^{3+}]\).
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