What is the ΔG for the following reaction at 25°C?

SO3 (g) + H2O (l) → H2SO4 (l)

Given:

SO3 (g) : ΔG = - 368 kJper mole

H2O (l) : ΔG = - 237 kJ per mole

H2SO4 (l) : ΔG = - 689.9 kJ per mole

84.9 kJ

558.9 kJ

-84.9 kJ

-558.9 kJ

Question

Krish Mathews

Chemistry

25 January, 11:57

What is the ΔG for the following reaction at 25°C?

SO3 (g) + H2O (l) → H2SO4 (l)

Given:

SO3 (g) : ΔG = - 368 kJper mole

H2O (l) : ΔG = - 237 kJ per mole

H2SO4 (l) : ΔG = - 689.9 kJ per mole

84.9 kJ

558.9 kJ

-84.9 kJ

-558.9 kJ

+2

Answers (1)

Know the Answer?

Braylen Hunter · Answer 1

We write the equation as:

-368 + - 237 = ΔH + - 689.9

ΔH = 84.9 kJ/mol

When written outside of the reaction equation, its sign will be reversed.

Thus, ΔH = - 84.9 kJ/mol

The third option is correct.

What is the ΔG for the following reaction at 25°C?SO3 (g) + H2O (l) → H2SO4 (l)Given:SO3 (g) : ΔG = - 368 kJper moleH2O (l) : ΔG = - 237 kJ per moleH2SO4 (l) : ΔG = - 689.9 kJ per mole84.9 kJ558.9 kJ-84.9 kJ-558.9 kJ

What is the ΔG for the following reaction at 25°C?

SO3 (g) + H2O (l) → H2SO4 (l)

Given:

SO3 (g) : ΔG = - 368 kJper mole

H2O (l) : ΔG = - 237 kJ per mole

H2SO4 (l) : ΔG = - 689.9 kJ per mole

84.9 kJ

558.9 kJ

-84.9 kJ

-558.9 kJ