The difference between ΔH and ΔU ( ΔH- ΔU), when the combustion of one mole heptane(I) is carried out a temperature T, is equal to:
-3RT
-4RT
3RT
4R
B.
-4RT
C7H16(l) + 11O2 → 7CO2 + 8H2O
Δngas = 7-11
ΔH = ΔU + ΔnRT
ΔH- ΔV = -4RT
Which of the following statement is correct for the spontaneous absorption of a gas?
For the reaction X2O4 (l) --> 2XO2 (g) ΔU = 2.1 kcal, ΔS = 20 cal K-1 at 300 K hence ΔG is
2.7 kcal
-2.7kcal
9.3 kcal
9.3 kcal
Which of the following statements is correct for a reversible process in a state of equilibrium?
ΔG = 2.303RT log K
ΔG0 = -2.303RT log K
ΔG0 = -2.303RT log K
The correct thermodynamic conditions for the spontaneous reaction at all temperatures is