1. At a certain temperature, the equilibrium constant for the following chemical

Question

1. At a certain temperature, the equilibrium constant for the following chemical equation is 2.80. At this temperature, calculate the number of moles of NO2(g) that must be added to 2.52 mol of SO2(g) in order to form 1.20 mol of SO3(g) at equilibrium.

SO2 (g) + NO2 (g) ---> SO3 (g) + NO (g)

2. At a certain temperature, the equilibrium constant, Kc, for this reaction is 53.3. At this temperature, 0.700 mol of H2 and 0.700 mol of I2 were placed in a 1.00-L container to react. What concentration of HI is present at equilibrium?

H2(g) + I2 (g) ---> 2HI (g) Kc= 53.3

Explanation / Answer

..........SO2 + NO2 ==> SO3 + NO
I.........2.53...0.......0.....0 1. At a certain temperature, the equilibrium constant for the following chemical equation is 2.80. At this temperature, calculate the number of moles of NO2(g) that must be added to 2.52 mol of SO2(g) in order to form 1.20 mol of SO3(g) at equilibrium.



SO2 (g) + NO2 (g) ---> SO3 (g) + NO (g)



2. At a certain temperature, the equilibrium constant, Kc, for this reaction is 53.3. At this temperature, 0.700 mol of H2 and 0.700 mol of I2 were placed in a 1.00-L container to react. What concentration of HI is present at equilibrium?



H2(g) + I2 (g) ---> 2HI (g) Kc= 53.3
C..........-x....x.......1.1...1.1
E.........2.53-x..x......1.1....1.1

Total mols = 2.53-x_x_1,1+1.1 = 4.73-x

XSO2 = (2.53-x)/(4.73-x)
XNO2 = x/(4.73-x)
XSO3 = 1.1/(4.73-x)
XNO = 1.1(4.73-x)

Then partial pressures are
pSO2 = (2.53-x)/(4.73-x)]*Ptotal
pNO2 = [x/(4.73-x)]*Ptotal
pSO3 = [1.1/(4.73-x)]*Ptotal
pNO = [1.1/4.73-x)]*Ptotal

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