Chem 1! For a particular reaction, ΔH = -14.20 kJ/mol and ΔS = -198.5 J/(mol·K). Calculate ΔG for this reaction at 298 K.?

I got -44.953 and I've redone the calculations several times and it's still wrong.

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  • Fern
    Lv 7
    1 year ago

    Delta G = -14.20 kJ/mole - 298(-0.198.5 kJ/moleK

    Delta G = -14.20 - (-59.15)

    Delta G = -14.20 + 59.15

    Delta G = +44.953 kJ

    Answer should be +44.95 kJ, not -44.95 kJ

    • Ally1 year agoReport

      thank you!

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  • 1 year ago

    Negative 43. 953?!? OH NO! YOU CREATED A BLACK HOOOOOOOOOOOOOOOOOOOOOOOOOOOOLLLLE!.............. or you have a dead battery (Sorry, I never took chemistry, I took anatomy instead. Just offering some humor during your hectic homework!)

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