laurence_hyde1
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The reaction I2(g) = 2I(g) was studied by sealing solid iodine, I2, in a glass bulb and measuring the total equilibrium pressure in the bulb at various temperatures (the I2 completely sublimes). The following data was obtained:
Volume of bulb= 249.8 ml; original mass of I2= 497 mg;
At T = 800C the total pressure was 0.738 atm
At T = 1000C the total pressure was 0.984 atm
a) Show that the equilibrium pressure of I2(g) is (2Po – Pt) and that of I(g) is 2(Pt - Po), where Po is the original pressure of I2(g) (at the particular temperature in question, when no decomposition occurs and Pt is the total pressure in the bulb at equilibrium. Assume ideal gas behaviour throughout.
b) Calculate Kp for each temperature.
c) Calculate deltaH in kJ mole for the reaction in the temperature range 80C to 1000 C (assume Ho is independent of temperature).
d) Calculate the free energy and entropy change for the reaction at 800C.
Volume of bulb= 249.8 ml; original mass of I2= 497 mg;
At T = 800C the total pressure was 0.738 atm
At T = 1000C the total pressure was 0.984 atm
a) Show that the equilibrium pressure of I2(g) is (2Po – Pt) and that of I(g) is 2(Pt - Po), where Po is the original pressure of I2(g) (at the particular temperature in question, when no decomposition occurs and Pt is the total pressure in the bulb at equilibrium. Assume ideal gas behaviour throughout.
b) Calculate Kp for each temperature.
c) Calculate deltaH in kJ mole for the reaction in the temperature range 80C to 1000 C (assume Ho is independent of temperature).
d) Calculate the free energy and entropy change for the reaction at 800C.