Question

What is the ΔG for the following reaction at 25°C?
N2O4(g) → 2NO2(g)
Given:
N2O4(g):ΔG= 98.28 kJ per mole
NO2(g):ΔG= 51.8 kJ per mole

5.32 kJ

10.64 kJ

–5.32 kJ

–10.64 kJ

Answer 1

@JFraser

Answer 2

what's the equation for calculating \(\Delta G\) when you have the \(Delta G\) of each reactant and each product?

Answer 3

N2O4(g) → 2NO2(g)?

Answer 4

I'm not sure what the equation would be.

Answer 5

it's something like \(\Sigma products\) - \(\Sigma reactants\)

Answer 6

not that one,

Answer 7

you're given the \(\Delta G\) of both substances, you just need to find the \(difference\) between them

Answer 8

I got -5.32

Answer 9

the order you subtract them in matters, and it's always \(products - reactants\)

since the \(NO_2\) is a product, you start with that, but there's 2 of them, so you take the \(\Delta G\) and double it\[2mol*(52kJ/mol)\] and then subtract the \(\Delta G\) of the reactant, \(N_2O_4\)\[2mol*(51.8kJ/mol)\ - 1mol*(98.28kJ/mol)\]

Answer 10

and I get a \(positive\) 5.32kJ

Answer 11

Oh, okay I see where I messed up.