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12 Dec 2019

At constant temperature and pressure, which statement gives the relationship between the sign of ÎG and the spontaneity of the reaction?

1) When ÎG < 0, the forward reaction is spontaneous.

2) When ÎG > 0, the forward reaction is spontaneous.

3) When ÎG < 0, the reverse reaction is spontaneous.

4) When ÎG = 0, the forward reaction is spontaneous.

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13 Dec 2019

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A process at constant T and P can be described as spontaneous if ÎG < 0 and nonspontaneous if ÎG > 0. Over what range of temperatures is the following process spontaneous? Assume that gases are at a pressure of 1 atm. (Hint: Use the data below to calculate ÎH and ÎS [assumed independent of temperature and equal to ÎHÂ° and ÎSÂ°, respectively] and then use the definition of ÎG.)

	2 SO₃(g)	â	2 SO₂(g)	+	O₂(g)
ÎH_fÂ° (kJ mol^-1)	-395.7		-296.8
SÂ° (J K^-1 mol^-1)	256.8		248.2		205.1

ÎHÂ° = kJ

ÎSÂ° = J K^-1

The calculated value of T at which ÎGÂ° = 0 is K.

Reaction is spontaneous _________above this temperaturebelow this temperatureat all temperaturesat no temperature.

Part A: Using the heats of formation and standard entropy, calculate ÎH0 and ÎS0 then use these to calculate ÎG0 and determine if the reaction is spontaneous at 1000C. If not, under what temperature conditions will it become spontaneous? and K at the given temperature. Assume ÎH0 and ÎS0 are not affected by temperature.

O2(g) + 2F2(g) <----> 2F2O(g) T= 1000C

ÎHf0(kJ/mol) 0 0 24.7

S0(J/K-mol) 205.2 202.8 247.43

Part B: Calculate equilibrium constant (K) and state whether products or reactants are favored

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	1) When ÎG < 0, the forward reaction is spontaneous.
	2) When ÎG > 0, the forward reaction is spontaneous.
	3) When ÎG < 0, the reverse reaction is spontaneous.
	4) When ÎG = 0, the forward reaction is spontaneous.