1. Consider the following reaction:
2 HI (g) → H
2 (g) + I
2 (g)
Assume that an experiment is carried out in which the starting concentration of HI (g) is 0.100 mol/L. No products are present at the beginning of the reaction. When equilibrium is established, the concentration of H
2 (g) is 1.73 x 10
-2 mol/L. Calculate the equilibrium constant for the above reaction.
2. The compound NOCl decomposes to nitric oxide and chlorine according to the following equation:
2 NOCl (g) → 2 NO (g) + Cl
2 (g)
Suppose that 0.810 mol NOCl is placed in a 4.00-L flask at a given temperature. When equilibrium has been established, it is found that the concentration of Cl
2 is 0.0105 M. Calculate the equilibrium constant for this reaction.
3. Nitrogen and oxygen react to produce nitric oxide according to the following equation:
N2 (g) + O2 (g) → 2 NO (g)
The equilibrium constant for this reaction is 1.70 x 10
-3. Suppose that 0.680 mol N
2 and 0.600 mol O
2 are mixed in a 2.00-L reaction vessel. What will be the concentrations of N
2, O
2, and NO when equilibrium is established? (Hint: assume that the amounts of N
2 and O
2 that react are small—less than 10% of the starting amounts—and check your assumption when you have solved the equation.)
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