Given the data: Ag2O (s), Delta Hf = -31.1kJ/mol, S = 121.3J/mol Ag (s), delta H

Question

Given the data: Ag2O (s), Delta Hf = -31.1kJ/mol, S = 121.3J/mol Ag (s), delta Hf = 0kJ/mol, S = 42.55J/mol K O2 (g), delta Hf = 0kJ/mol, S = 205J/mol K
Calculate the temperature at which delta delta G = 0 for the reaction, Ag2O -> 2Ag + 1/2 O2
Assume that, since the physical states do not change, delta H and delta S are independent of temperature between -50C and 950C.
A) 196C * B) 246C C) 423C D) 610C E) 818C Given the data: Ag2O (s), Delta Hf = -31.1kJ/mol, S = 121.3J/mol Ag (s), delta Hf = 0kJ/mol, S = 42.55J/mol K O2 (g), delta Hf = 0kJ/mol, S = 205J/mol K
Calculate the temperature at which delta delta G = 0 for the reaction, Ag2O -> 2Ag + 1/2 O2
Assume that, since the physical states do not change, delta H and delta S are independent of temperature between -50C and 950C.
A) 196C * B) 246C C) 423C D) 610C E) 818C Given the data: Ag2O (s), Delta Hf = -31.1kJ/mol, S = 121.3J/mol Ag (s), delta Hf = 0kJ/mol, S = 42.55J/mol K O2 (g), delta Hf = 0kJ/mol, S = 205J/mol K
Calculate the temperature at which delta delta G = 0 for the reaction, Ag2O -> 2Ag + 1/2 O2
Assume that, since the physical states do not change, delta H and delta S are independent of temperature between -50C and 950C.
A) 196C * B) 246C C) 423C D) 610C E) 818C

Explanation / Answer

We calculate delta H and delta S of the given reaction.

Reaction :

Ag2O --- > 2 Ag + ½ O2

Delta Hrxn = [2 mol * Delta H Ag + ½ mol * delta H O2 ]- [ 1 mol * delta H of Ag2O ]
=2 mol * 0 + ½ mol * 0 ] – [-31.1 kJ/mol ]

= +31.1 kJ= 31100 J

Delta S = [2 mol * Delta S Ag + ½ mol * delta S O2 ]- [ 1 mol * delta S of Ag2O ]
= [2 mol * 42.55 J per mol per K + ½ mol * 205 J per mol per K ]

We know when Delta G is 0 then equation becomes

0 = delta H – Tdelta S

Delta H = T delta S

T = Delta H / delta S

= 31100 J /66.3 J per K

=469.1 K

Lets convert this into deg C

= 469.1 – 273.15 = 195.93

= 196 deg C

And answer is option a) = 196 deg C

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