Consider the reaction at 298 K. 4NO2(g)+O2(g)↽−−⇀2N2O5(g) Calculate Δ𝐺∘rxn to demonstrate that the reaction is n
Posted: Tue Nov 16, 2021 6:34 am
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 N2O5 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
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 N2O5 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