Question

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

Answer 1

Do you know what triangleG means?

Answer 2

It's supposed to represent change over time

Answer 3

the "triangle" is the uppercase greek letter delta, \(\Delta\).

it means "change" but not with respect to time

Answer 4

So for the question, you'd use

\(\sf \huge \Delta G_{reaction}=\Delta G _{products}-\Delta G_{reactants}\)

Answer 5

@aaronq okay, but which ones are the products and which are the reactants?

Answer 6

Is that the whole question?

Answer 7

@Ajohnson2199 yes, the bottom four are the possible answers.

Answer 8

Okay, so I'm pretty sure that what the chemical equation yields are the products

Answer 9

So, H2SO4 is the product

Answer 10

And the reacts are SO3 + H2O

Answer 11

You following me?

Answer 12

@Ajohnson2199 okay so how would I put that into an equation?

Answer 13

Well, just plug in the numbers.

Answer 14

@Ajohnson2199 the answer is 84.9?

Answer 15

Did you check your work?