A) The reaction is only spontaneous at low temperatures. B) The reaction is spon

Question

A) The reaction is only spontaneous at low temperatures.

B) The reaction is spontaneous at all temperatures.

D) The reaction is spontaeous only at high temperatures

For the reaction H2(g) + S(s) 25 degree C under standard conditions Delta G degree becomes less favorable as temperature increases. D) The reaction is spontaeous only at high temperatures E) The reaction is at equilibrium at delta S degree = +43.1kJ.mol. Which of these statements is true? A) The reaction is only spontaneous at low temperatures. B) The reaction is spontaneous at all temperatures. C) delta H degree = -20.2 kJ/mol and H2S(g),

Explanation / Answer

option B is correct

because delta G = delta H - T delta S for spontaneous reaction delta G should be negative delta H is negative and delta S is postive the whole expression is negative at any temperature that means delta G is < 0 at any Temperature

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