For which reaction, carried out at standard conditions, wouldboth the enthalpy a

Question

For which reaction, carried out at standard conditions, wouldboth the enthalpy and entropy changes drive the reaction in thesame direction? Please EXPLAIN. A. 2H2(g) + O2(g) --->2H2O(l)         H = -571.1 kJ B. 2Na(s) + Cl2(g)---->2NaCl(s)       H = -822.0kJ C. N2(g) + 2O2(g) ---->2NO2(g)       H= +67.7 kJ D. 2NH3(g) ----> N2(g) +3H2(g)        H= +92.4 kJ For which reaction, carried out at standard conditions, wouldboth the enthalpy and entropy changes drive the reaction in thesame direction? Please EXPLAIN. A. 2H2(g) + O2(g) --->2H2O(l)         H = -571.1 kJ B. 2Na(s) + Cl2(g)---->2NaCl(s)       H = -822.0kJ C. N2(g) + 2O2(g) ---->2NO2(g)       H= +67.7 kJ D. 2NH3(g) ----> N2(g) +3H2(g)        H= +92.4 kJ

Explanation / Answer

Entropy increases when # of molecules in a system increaes. Areaction would occur spontaneously if the enthalpy value isnegative. A. Entropy drives the reaction to shift towardthe reactants (toward increasing the number of molecules) andthe enthalpy since its negative, drives the reaction to go towardthe products. they are not driving the reaction in the samedirection, so A is not the right answer. B. Entropy wants the reaction to shift towardthe reactants (toward increasing the number of molecules) andthe enthaply is a large negative number so the reaction willproceed toward the products. they are not in the same direction andB is not he right answer. C. Entropy would drive the reaction to shift towardthe reactants (toward increasing the number of molecules) andthe + enthalpy value would drive the reaction towardreactants. therefore this is the right answer because both entropyand enthalpy are driving the reaction in the samedirection. D. Entropy wants the reaction to shift toward products (towardincreasing the number of molecules) and the + enthalpy value woulddrive the reaction toward the reactants. therefore D is not theright answer. Hope that helps

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