Question

Part A:

For the reaction

CO(g) + 3H₂(g) ---> CH₄(g) + H₂O(g)

(delta)H° = -206.1 kJ and (delta)S° = -214.7 J/K

The standard free energy change for the reaction of 1.54 moles of CO(g) at 293 K, 1 atm would be (?) kJ.

This reaction is (reactant, product)(?) favored under standard conditions at 293 K.

Assume that (delta)H° and (delta)S° are independent of temperature.

Part B:

For the reaction

I₂(g) + Cl₂(g) --> 2 ICl(g)

(delta)G° = -30.0 kJ and (delta)S° = 11.4 J/K at 282 K and 1 atm.

This reaction is (reactant, product)(?) favored under standard conditions at 282 K.

The standard enthalpy change for the reaction of 1.74 moles of I₂(g) at this temperature would be (?) kJ.
Part C:

For the reaction

2 HBr(g) --->  H₂(g) + Br₂(l)

(delta)G° = 110.3 kJ and (delta)H° = 72.6 kJ at 329 K and 1 atm.

This reaction is (reactant, product)(?) favored under standard conditions at 329 K.

The entropy change for the reaction of 1.57 moles of HBr(g) at this temperature would be (?) J/K.

Answer 1