# Problem: For each of the following reactions, calculate ΔH°rxn, ΔS°rxn, and ΔG°rxn at 25 °C. State whether or not the reaction is spontaneous. If the reaction is not spontaneous, would a change in temperature make it spontaneous? If so, should the temperature be raised or lowered from 25 ∘C?Part G N2(g)+O2(g)→2NO(g) Express your answer using three significant figures.ΔH°rxn = kJPart H Calculate ΔS°rxn at 25 °C. Express your answer to one decimal place.ΔS°rxn = J/K

###### FREE Expert Solution

We’re being asked to determine the standard enthalpy change (ΔH˚rxn) for the balanced reaction:

N2(g)+O2(g)→2NO(g)

Recall that ΔH˚rxn can be calculated from the enthalpy of formation (ΔH˚f) of the reactants and products involved:

The ΔH˚f values: can be found in books or online:

ΔH˚f NO(g) = 90.25  kJ/mol
ΔH˚f O2(g) 0 kJ/mol (ΔH˚f = 0 for elements in their standard state)
ΔH˚f N2(g) 0 kJ/mol (ΔH˚f = 0 for elements in their standard state)

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###### Problem Details

For each of the following reactions, calculate ΔH°rxn, ΔS°rxn, and ΔG°rxn at 25 °C. State whether or not the reaction is spontaneous. If the reaction is not spontaneous, would a change in temperature make it spontaneous? If so, should the temperature be raised or lowered from 25 ∘C?