Consider this reaction occurring at 298 K: N2O(g) + NO2(g) à 3 NO(g) DG0 f (N2O(g)) = 103.7 kJ, DG0 f (NO2(g)) = 51.3 kJ, and DG0 f (NO(g)) = 87.6 kJ a. Show that the reaction is not spontaneous under standard conditions by calculating DGo rxn. b. If a reaction mixture contains only N2O and NO2 at partial pressures of 1.0 atm each, the reaction will be spontaneous until some NO forms in the mixture. What maximum partial pressure of NO builds up before the reaction ceases to be spontaneous?c. Can the reaction be made more spontaneous by an increase or decrease in temperature? If so, what temperature is required to make the reaction spontaneous under standard conditions?

Ithe undersigned only for use your own email and delete any and copies and of the itself and to be there is a good timewhat does a decrease in temperature indicate about the molecules in a sample of liquid water? decreased chemical energy of the moleculesdecreased kinetic energy of the moleculesincreased chemical energy of the moleculesincreased kinetic energy of the moleculeshow does a sample of helium at 15 â°c compare to a sample of helium at 215 k? the helium at 15 â°c has a higher average kinetic energy than the sample at 215 k.the helium at 15 â°c has lower nuclear energy than the sample at 215 k.the helium at 15 â°c has slower-moving atoms than the sample at 215 k.the helium at 15 â°c has smaller atoms than the sample at 215 k.

Ibelieve the answer is b.2200 watts, because p=vi; p=220(10); then p=2200hope my answer has you : )