Given the following Thermodynamic data: CO2(g) H2O(l) NH3(g) CO(NH2)2(s) DeltaHof (kJ/mol): -393.5 -285.85 -45.9 -333.2 So...

Question

Question

Given the following Thermodynamic data:

CO_2(g) H₂O_(l) NH_3(g) CO(NH₂)_2(s)

DeltaH^of (kJ/mol): -393.5 -285.85 -45.9 -333.2

S^o (J/K.mol): 214 70 193 105

(a) Calculate DeltaH^o, DeltaS^o, and DeltaG^o at 25^oC for the following reaction:

CO2(g) + 2NH3(g) = CO(NH₂)_2(s) + H2O_(l)

(b) What is DeltaG^o at 250^oC? (Assume DeltaH^o and DeltaS^o do not change with temperature.)

(c) Is the reaction spontaneous at each temperature?

(Answer: (a) DeltaH^o = -133.8 kJ; DeltaS^o = -425 J/K; DeltaG^o = -7.15 kJ; (b) DeltaG^o = 88.5 kJ;

(c) Reaction is spontaneous at 25^oC but not at 250^oC.)

science chemistry

Answer 1

Answer #1

For a reaction to be spontaneous, G_r is supposed to be negative.

At 25⁰C, G_r is negative, thus the reaction is spontaneous

At 250⁰C, G_r is positive, thus the reaction is not spontaneous

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Answer 2

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