Question

I'm a bit confused with the options. My answer is not matching with it. Need help!! question no. 47

Answer 1

hello mate

use this formula..
2A(g) + B(g) -------> 2C(g) : ΔU° = -10.0 KJ
Δng = np - nr 
       = 2 - (2 + 1) = 2 - 3 = -1 

ΔH° = ΔU° + ΔΔngRT,  from formula,
       = -10.0 KJ + (-1) × 0.008314 KJ/K/mol × 298K
       =-10.0 KJ - 2.447 KJ
       = -12.447 KJ
now, use the formula, ΔG° = ΔH° - TΔS°
                                           = -12.447 KJ - 298K × (-45 × 10⁻³ J/K)
                                           = -12.447 KJ + 13.41 KJ
                                           = + 0.930 KJ or 930 JOULE ( approximately)
the reaction will not occur spontanteously because ΔG° is positive.
so the answer is 1

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Answer 2

(1) +930 J/mol.

Given is just ∆U.

∆H at 298K = ∆U + ∆PV = ∆U - RT (using ∆ng of reaction)

∆H = -10000J -2477.572J = -12477.572J

(using R = 8.314, T = 298)

∆G = ∆H - T∆S, and proceeding as you probably did with the above value of ∆H, we'll get:

∆G = +932.428 J/mol.