Here it says the given reaction has a change in the standard Gibbs free energy of -374 kilojoules and partial pressures of sulfur. Tetrafluoride, fluorine gas and sulfur hexafluoride are .63 atmospheres, 0.95 atmospheres and 1.7 atmospheres respectively. Here we need to calculate the change in the non standard Gibbs free energy of the reaction for this reaction.

So here is our balanced equation. It's a one to one relationship with everything. Here we're going to say that ΔG equals ΔG₀ or not plus RTlnQ. Here they're giving us these values. They're going to help us find Q. Just like an equilibrium constant is equal to products over reactants. It ignores solids and liquids, but everything here is a gas.

So it equals the pressure of sulfur hexafluoride divided by the pressure of sulfur tetrafluoride times the pressure of fluorine gas. Plug in the value, so we have 1.7 divided by 0.63 * 0.95. Q here equals 2.84, so we have what our Q is. We have what ΔG₀ is. Here R uses joules, so we're going to convert these kilojoules into joules by multiplying them by 1000.

When we do that we get -374000 Joules plus 8.314 Joules over moles times K. Here temperature were not given a temperature so we're assuming it's under standard temperature which is 298.15 Kelvin and then we have ln of Q which is 2.840. When we plug all this in, this will give us the change in the non standard Gibbs free energy which comes out to -3.71 * 10⁵ joules. OK, so this would be our final answer for this given question.