Consider the reaction at 298 K. 4NO2(g)+O2(g)↽−−⇀2N2O5(g) Calculate Δ𝐺∘rxn to demonstrate that the reaction is n

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Consider the reaction at 298 K.
4NO2(g)+O2(g)↽−−⇀2N2O5(g)
Calculate Δ𝐺∘rxn to demonstrate that the reaction is
nonspontaneous under standard conditions. Thermodynamic properties
can be found in this table.
Δ𝐺∘rxn= 29000J/mol
If a reaction begins with a mixture of NO2 and O2 at partial
pressures of 1.00 atm each, the reaction will be spontaneous until
some N2⁢O5 forms in the mixture. What is the maximum partial
pressure of N2O5 that can build up before the reaction ceases to be
spontaneous?
𝑃N2O5= atm
Can the reaction be made more spontaneous by an increase or a
decrease in temperature?
increase
decrease
What temperature is required to make the reaction spontaneous
under standard conditions?
T= K