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What is Gibbs Free Energy?

Gibbs Free energy for reaction under standard conditions!! Help!!?

  • Calculate Gibbs free energy change in kj for the reaction below at 25C, when the pressures of N2, H2, and NH3 are 2.50 atm, 4.62 atm, and .0305 atm, respectively. (I have the thermodynamic data if needed Just give me steps please!) N2(g) + 3H2(g) ----->< 2NH3(g) Okay. I know I have to solve for the eq.constant, don't I? I don't want an answer, just please guide me through solving this problem! Also, this other problem has me very confused. Calculate the gibbs free energy change in kj for the process below at 210C when the pressures of H2, CL2, and HCL are .00850 atm, .0600 atm, 40.0 atm respectively. (Once again, I have thermodynamic data). H2+CL2--------------><2HCL For this second problem I calculated delta s and delta h and plugged it into the equation deltaG=deltaG0+RT*lnQ but still had the wrong answer... PLEASE HELP! thank you!!!

  • Answer:

    First one--yes! Use PV = nRT to solve for the number of moles of each (remember that the gases are all in the same volume, so you can set V to whatever you want), and then use the number of moles to get K. Once you have that, use deltaG = -RT log K to solve for delta G. Same for the second one.

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First one--yes! Use PV = nRT to solve for the number of moles of each (remember that the gases are all in the same volume, so you can set V to whatever you want), and then use the number of moles to get K. Once you have that, use deltaG = -RT log K to solve for delta G. Same for the second one.

Mark S, JPAA

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