Assuming H and S do not vary with temperature, atwhat temperature will the react

Question

Assuming H and S do not vary with temperature, atwhat temperature will the reaction shown below becomespontaneous? C(s) +H2O(g)------------>CO(g) +H2(g) H=11.3kJ                         S=133.6J/K A. Below 710degC       B.above983deg C     C. above 710degC    D. above 1 deg C. E. below 983 degC. Show work! Assuming H and S do not vary with temperature, atwhat temperature will the reaction shown below becomespontaneous? C(s) +H2O(g)------------>CO(g) +H2(g) H=11.3kJ                         S=133.6J/K A. Below 710degC       B.above983deg C     C. above 710degC    D. above 1 deg C. E. below 983 degC. Show work!

Explanation / Answer

The reaction is spontaneous if and only if change in Gibb'sfree energy is less than ZERO G < 0 But G = H - T S So , H - T S < 0   ===>   H < TS     ===>   H /S < T             11.3* 1000 J / 133.6 J / K < T                84.58 < T So the temperature is greater than 84.58 K = 84.58 - 273= -188.42 oC

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