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Calculate the temperature above which the given reaction become spontaneous. `C_((s)) + H_(2)O_((g)) rarr CO_((g)) + H_(2(g))` `DeltaH^(@) = + 131.3 KJ//"mole"` , `DeltaS^(@) = + 0.1336 KJ//"mole" K`A. `98.8 K`B. `709.8^(@)C`C. `491.4 K`D. `354.9^(@)C` |
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Answer» Correct Answer - B `Delta G = DeltaH - TDeltaS` `0 = +131.3 - T(+0.1336)` (for spontaneity) `T gt (131.3)/(0.1336) = 982.8 K` `t^(@)C gt 982.8 - 273 = 709 .8^(@)C` |
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