The table below lists the equilibrium concentrations for H _{2}(g), I_{2}(g), and HI(g) in the given reaction.

H_{2 }(g) + I_{2 }(g) ⇌ 2HI (g)

At 500 K, the gases have equilibrium partial pressures of P_{I2} = 1.00 atm, P_{H2 }= 1.00 atm, and P_{HI }= 0.0795 atm. An addition of 0.100 atm HI(g) is made to this system.

Determine the final partial pressures for H_{2}(g), I_{2}(g), and HI(g) when the system returns to equilibrium (i.e., after the addition of 0.100 atm HI(g)).

a. P_{I2} = 1.086 atm, P_{H2 }= 1.086 atm, and P_{HI }= 0.00695 atm

b. P_{I2} = 1.275 atm, P_{H2 }= 1.275 atm, and P_{HI }= 0.0225 atm

c. P_{I2} = 1.621 atm, P_{H2 }= 1.621 atm, and P_{HI }= 0.00731 atm

d. P_{I2} = 1.072 atm, P_{H2 }= 1.072 atm, and P_{HI }= 0.00642 atm

e. P_{I2} = 1.372 atm, P_{H2 }= 1.372 atm, and P_{HI }= 0.00614 atm

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