Given the reaction: 2 Cl2 (g) + 2 H2O (g) ⇌ 4 HCl (g) + O2 (g) Kp = 7.5x10-2, calculate the Gibbs Free Energy change for the reaction below at 30ºC. 8 HCl (g) + 2 O2 (g) ⇌ 4 Cl2 (g) + 4 H2O (g)

Here it says, given the reaction where we have 2 moles of chlorine gas reacting with 2 moles of water vapor to produce 4 moles of hydrogen chloride, plus 1 mole of oxygen gas. We were told that our equilibrium constant is equal to 7.5 times 10 to the negative 2. We need to calculate the Gibbs free energy change for the reaction below at 30 degrees Celsius. Alright, so they're giving us k, they're giving us temperature, and they want us to find Gibbs free energy. Now remember, there are 2 equations that can connect together our equilibrium constant to Gibbs free energy. Those equations are equilibrium constant equals the inverse of the natural log to the negative delta g zero divided by RT. We'd use this version if we need to find our equilibrium constant, but now we need to find Gibbs free energy instead. So another way of writing the same equation is the change in our standard Gibbs free energy equals negative RT ln of k. This is the version we're going to use because we need to find our Gibbs free energy at the end. R here is going to be 8.314 joules over moles times k. This is our gas constant. Temperature needs to be in Kelvin, so add 273.15 to our degrees Celsius to give us 303.15 Kelvin. And then we just plug in ln of k, so ln of 7.5 times 10 to the negative 2. When we work this out, we're gonna get negative one 3057.38 joules over moles because our Kelvins cancel out. Now, here, we can go with 2 sig figs. We'll do negative 1.3 times 10 to the 4 joules per mole. This would be our final answer for this question.

Given the reaction: 2 Cl2 (g) + 2 H2O (g) ⇌ 4 HCl (g) +...

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Given the reaction: 2 Cl2 (g) + 2 H2O (g) ⇌ 4 HCl (g) + O2 (g) Kp = 7.5x10-2, calculate the Gibbs Free Energy change for the reaction below at 30ºC.8 HCl (g) + 2 O2 (g) ⇌ 4 Cl2 (g) + 4 H2O (g)

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Given the reaction: 2 Cl2 (g) + 2 H2O (g) ⇌ 4 HCl (g) + O2 (g) Kp = 7.5x10-2, calculate the Gibbs Free Energy change for the reaction below at 30ºC.
8 HCl (g) + 2 O2 (g) ⇌ 4 Cl2 (g) + 4 H2O (g)