Given: SO₂(g) →O₂(g)+ S(s) K_c = 2.5 * 10^-53 SO₃(g) → O₂(g)+ SO₂(g) K_c = 4.0 * 10^-13 Calculate K_c for the reaction 2S(s)+ 3O₂(g) →2SO₃(g)

Question

Quizplus · Accepted Answer

We can use the equation: 
ΔG° = - RTln(K)
Where ΔG° is the standard free energy change, R is the gas constant and T is the temperature in Kelvin. 
We assume the reaction to be taking place at standard conditions, so ΔG° = 0.
Thus, we have:
0 = - RTln(K)
ln(K) = 0
K = 1
We substitute the values given for KS1U1B1cS1U1B0 for the reactants and products:
K = (KS1U1B1cS1U1B0)^2 / (KS1U1B1cS1U1B0)^3 (KS1U1B1cS1U1B0)
1 = (KS1U1B1cS1U1B0)^-1
KS1U1B1cS1U1B0 = 1
However, we are given answer choices in the form of 10 raised to a certain power. Thus, 
KS1U1B1cS1U1B0 = 1 = 10^0
10S1U1P1130 S1S1P0 = 10^1.630 S1S1P0
10S1U1P165 S1S1P0 = 10^1.217 S1S1P0
10S1U1P1103 S1S1P0 = 10^3.042 S1S1P0
10S1U1P140 S1S1P0 = 10^1.146 S1S1P0
10S1U1P180 S1S1P0 = 10^0.827 S1S1P0
Thus, the best choice is C, 1.0 F1F1F1S1F1F1F10 10S1U1P1130 S1S1P0.

Given: SO2(g) →O2(g)+ S(s)

Given: SO₂(g) →O₂(g)+ S(s)