Chemistry - Science (Dr. Bob222)

The following reaction has a positive value of ΔG°.
2H2O(g) → 2H2(g) + O2(g)
Which of the following statements must be true?
A. The reaction is slow.
B. The reaction will not occur. That is, when H2O(g) is introduced into a flask, no O2 or H2 will form
even over a long period of time.
C. The reaction is exothermic.
D. The equilibrium lies far to the right.
E. None of these is true.

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asked by Ana
  1. Hello, how are you?
    The correct answer to this Q is E. but I have chosen B. Could you please explain why all of them cannot be true? Thank you

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    posted by Ana
  2. A. dG has nothing to do with speed of a reaction. Carbon is the more stable form of diamond but all the girls getting diamond rings today need not worry about that ring crumbling tomorrow. :-).
    B. All reactions occur to some extent no matter how small. So this has an extremely small Keq, so it's small but still occurs.
    C. Is the reaction exothermic. I thought the reverse reaction was exothrmic.
    D. No, the eq lies far to the left; otherwise all of our lakes and rivers would have dried up long ago and we would have plenty of oxygen and hydrogen in our atmosphere.
    E. That leaves E.

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    posted by DrBob222
  3. Thank you!

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    posted by Ana

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