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28 February, 00:10

For the reaction below G° = + 33.0 kJ, H° = + 92.2 kJ, and S° = + 198.7 J/K. Estimate the temperature (K) at which this reaction becomes spontaneous. 2 NH3 (g) → N2 (g) + 3 H2 (g)

a) 0.464k b) 166k c) 214k d) 298k e) 464k

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Answers (2)
  1. 28 February, 02:08
    0
    D

    Explanation:

    A reaction becomes spontaneous when the value of the change in free energy is negative.

    The relationship between the enthalpy, the entropy and the free energy in a chemical reaction is given below:

    G = H - TS

    Now, let's input the values that we have.

    One important thing to note is that we have to convert the KJ to Joules and this mean we have to multiply by a conversion factor of 1000. This mean 33KJ is 33,000J

    33,000 = 92,200 - 198.7T

    33,000 - 92,200 = - 198.7T

    -59,200 = - 198.7T

    T = 59,200/198.7

    T = 298k
  2. 28 February, 03:46
    0
    464K

    Explanation:

    △G° = △H° - T△S°,

    33 = 92.2 - T (198.7/1000) [divide by 1000 to convert J to kJ]

    T = (92.2 - 33) / (198.7/1000) = 298K

    If reaction is spontaneous, △G° has to be negative, so

    0 = △H° - T△S°

    T = △H°/△S° = 92.2 / (198.7/1000) = 464K
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