Question

5 mol h2o at 100 c and 1 atm is converted into h2o at 100 c and 5 atm the delta g i

Answer 1

Hey buddy,

● Answer-
∆G° = 24965 J

● Exlaination-
# Given-
n = 5 mol
T = 100 ℃ = 373 K
P1 = 1 atm
P2 = 5 atm

# Solution-
Gibbs free energy change is given by-
∆G° = nRT ln(P2/P1)
∆G° = 5 × 8.314 × 373 × ln(5/1)
∆G° = 15506 × 1.61
∆G° = 24965 J

Hope this is helpful...

Answer 2

Explanation:

Delta G is known as Gibb's free energy and its relation with number of moles, pressure, temperature is as follows.

       $\Delta G = nRT \times ln(\frac{P_{2}}{P_{1}})$

The given data is as follows.

   n = 5 mol

   R = 8.314 J/mol

   T = 100 + 273 = 373 K

   $P_{1}$ = 1 atm,  $P_{2}$ = 5 atm

Therefore, putting the given data in the formula above as follows.

        $\Delta G = nRT \times ln(\frac{P_{2}}{P_{1}})$

                              = $5 mol \times 8.314 J/mol \times 373 K ln(\frac{5}{1})$

                               = $15505.61 \times 1.609$

                               = 24948.52 J K

Thus, we can conclude that value of $\Delta G$ = 24948.52 J k.