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1. For the reaction: N2(g) + O2(g)=2NO(g), deltaH° = 181 kJ and deltaS° = 24.9 J/K,...

1. For the reaction: N2(g) + O2(g)=2NO(g), deltaH° = 181 kJ and deltaS° = 24.9 J/K, deltaG° would be negative at temperatures (above, below) ?????K.
Enter above or below in the first box and enter the temperature in the second box. Assume that deltaH° and deltaS° are constant.

2. For the reaction: 2BrF3(g)=Br2(g) + 3F2(g), deltaH° = 542 kJ and deltaS° = 269 J/K, G° would be negative at temperatures (above, below)  K.
Enter above or below in the first box and enter the temperature in the second box. Assume that deltaH° and deltaS° are constant.

3. Consider the reaction
2CO2(g) + 5H2(g)=C2H2(g) + 4H2O(g)
Using the standard thermodynamic data in the tables linked above, calculate deltaG for this reaction at 298.15K if the pressure of each gas is 12.19 mm Hg.
ANSWER: ????? (kJ/mol)

4. Consider the reaction:
CO(g) + 3H2(g)=CH4(g) + H2O(g)
Using the standard thermodynamic data in the tables linked above, calculate deltaG for this reaction at 298.15K if the pressure of each gas is 19.60 mm Hg.
ANSWER: ?????? (kJ/mol)

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