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Homework 2

1 .       Write the expression for Keq for the following reaction:

Ti(s) + 2Cl2(g) TiCl4(l)

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2 .       Write the equilibrium constant for the heterogeneous reaction 2NaHCO3(s) Na2CO3(s) + CO2(g) + H2O(g).

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3 .       The proper expression for Keq for the reaction NiCO3(s) + 2H+(aq) Ni2+(aq) + CO2(g) + H2O(l) is

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4 .       What would be the correct equilibrium constant expression for the reaction
AgCl(s) + 2 NH3(aq) [Ag(NH3)2]+(aq) + Cl-(aq)?

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5 .       Gaseous hydrogen iodide is placed in a closed 1.0-L container at 425°C, where it partially decomposes to hydrogen and iodine:

2HI(g) H2(g) + I2(g). At equilibrium it is found that PHI = 3.53 x 10-3 atm; PH2 = 4.79 x 10-4 atm; and PI2 = 4.79 x 10-4 atm. What is the value of Keq at this temperature?

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6 .       Consider the reaction 2HI(g) H2(g) + I2(g).

What is the value of the equilibrium constant, Keq, if at equilibrium PH2 = 6.50 x 10-7 atm, PI2 = 1.06 x 10-5 atm, and PHI = 1.87 x 10-5 atm?

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7 .       Calculate the equilibrium constant for the reaction below if a 3.25-L tank is found to contain 0.343 atm O2, 0.0212 atm SO3, and 0.00419 atm SO2.

2SO3(g) 2SO2(g) + O2(g)

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8 .       A mixture of H2, S, and H2S is held in a 1.0-L vessel at 90°C until the following equilibrium is achieved:

H2(g) + S(s) H2S(g)

At equilibrium the mixture contains 0.46 g of H2S and 0.40 g H2. What is the value of Keq for the reaction at this temperature?

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9 .       A mixture of 0.1000 atm of CO2, 0.05000 atm of H2, and 0.1000 atm of H2O is placed in a 1.000-L vessel. The following equilibrium is established:

CO2(g) + H2(g) CO(g) + H2O(g).

At equilibrium PCO2 = 0.0954 atm. Calculate the equilibrium partial pressures of H2, CO, and H2O.

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10 .       A mixture of 0.100 atm of NO, 0.0500 atm of H2, and 0.100 atm of H2O is placed in a 1.00-L vessel at 300 K. The following equilibrium is established:

2NO(g) + 2H2(g) N2(g) + 2H2O(g)

At equilibrium PNO = 0.0620 atm.
Calculate the equilibrium partial pressures of H2, N2, and H2O.

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11 .       C6H6(g) + 3H2(g) C6H12(g). When 1.00 mol C6H6 and 3.00 mol H2 are put into a 200-L container and allowed to reach equilibrium over a catalyst at an elevated temperature, the resulting mixture contains 0.137 mol C6H12. What is the equilibrium amount of H2 in moles?

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12 .       Consider the reaction N2O4(g) 2NO2(g). Determine the value of the equilibrium constant for this reaction if an initial partial pressure of N2O4(g) of 0.0400 atm is reduced to 0.0055 atm at equilibrium. (There is no NO2(g) present at the start of the reaction.)

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