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=800 ‘C the total pressure was 0.738 atm
At T = 1000 ‘C the total pressure was 0.984 atm
a)Show that the equilibrium pressure of I2(g) is 2Po – Pt and that the I(g) is 2(Pt – Po), where Po is the original pressure of I2(g)(at the particular temperature in question, when no decomposing occurs) and Pt is total pressure in the bulb at equilibrium. Assume ideal gas behavior throughout.
b)Calculate Kp for each temperature.
c)Calculate ▲H’ in kj mole-1 for the reaction in the temperature range 800 ‘C to 100’C (assume ▲H’ is independent of temperature)
d)Calculate the free energy and entropy change for the reaction at 900 ‘C
the ' represents degrees
Volume of bulb = 249.8 ml; original mass of I2= 497 mg;
At T=800 ‘C the total pressure was 0.738 atm
At T = 1000 ‘C the total pressure was 0.984 atm
a)Show that the equilibrium pressure of I2(g) is 2Po – Pt and that the I(g) is 2(Pt – Po), where Po is the original pressure of I2(g)(at the particular temperature in question, when no decomposing occurs) and Pt is total pressure in the bulb at equilibrium. Assume ideal gas behavior throughout.
b)Calculate Kp for each temperature.
c)Calculate ▲H’ in kj mole-1 for the reaction in the temperature range 800 ‘C to 100’C (assume ▲H’ is independent of temperature)
d)Calculate the free energy and entropy change for the reaction at 900 ‘C
the ' represents degrees