For each reaction, calculate ΔH°_rxn, ΔS°_rxn, and ΔG°_rxn at 25°C and determine whether the reaction is spontaneous. If the reaction is not spontaneous, could a change in temperature make it spontaneous? If so, should the temperature be increased or decreased from 25°C? b. 2 NH3(g) → N2H4(g) + H2(g)

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1. <insert step 1: Write the balanced chemical equation for the reaction: 2 \text{NH}_3(g) \rightarrow \text{N}_2\text{H}_4(g) + \text{H}_2(g)>
2. <insert step 2: Use standard enthalpies of formation (\Delta H^\circ_f) to calculate \Delta H^\circ_{rxn}. The formula is \Delta H^\circ_{rxn} = \sum \Delta H^\circ_f(\text{products}) - \sum \Delta H^\circ_f(\text{reactants}).>
3. <insert step 3: Use standard molar entropies (S^\circ) to calculate \Delta S^\circ_{rxn}. The formula is \Delta S^\circ_{rxn} = \sum S^\circ(\text{products}) - \sum S^\circ(\text{reactants}).>
4. <insert step 4: Calculate \Delta G^\circ_{rxn} using the Gibbs free energy equation: \Delta G^\circ_{rxn} = \Delta H^\circ_{rxn} - T\Delta S^\circ_{rxn}, where T is the temperature in Kelvin (298 K for 25^\circ C).>
5. <insert step 5: Determine spontaneity by checking the sign of \Delta G^\circ_{rxn}. If \Delta G^\circ_{rxn} < 0, the reaction is spontaneous. If \Delta G^\circ_{rxn} > 0, consider how temperature affects spontaneity: if \Delta H^\circ_{rxn} > 0 and \Delta S^\circ_{rxn} > 0, increasing temperature may make the reaction spontaneous.>