Question

For the following questions, use the reaction NO2(g) N2(g) + O2(g), with ΔH = –33.1 kJ/mol and ΔS= 0.06302 kJ/(mol·K).

i. Draw a possible potential energy diagram of the reaction. Label the enthalpy of the reaction.












ii. Is the reaction endothermic or exothermic? Explain your answer.








iii. What is the Gibbs free energy of the reaction at 298 K?







iv. Is the reaction spontaneous or nonspontaneous at 298 K? Explain your answer.





@thomaster @ash2326

Answer 1

@asnaseer @bahrom7893

Answer 2

when \(\Delta\)G is negative, by definition, your reaction is spontaneous, and when \(\Delta\)G is positive, reaction is nonspontaneous. To solve for \(\Delta\)G

\(\Delta\)G = \(\Delta\)H-T\(\Delta\)S

You are already given your numbers, simply plug and solve.

Answer 3

and your reaction is exothermic, your \(\Delta\)H value is negative, meaning that energy is being released into your system. If your value for \(\Delta\)H been positive, you would have a endothermic reaction.

Answer 4

Just to be clear, a system that releases heat to the surroundings is an exothermic reaction, this means your \(\Delta\)H is negative! because the enthalpy of the products is lower than the enthalpy of the reactants of the system.
On the otherhand, a system that absorbs heat from the surroundings is endothermic. The value is positive for \(\Delta\)H because the enthalpy of the products is higher than the enthalpy of the reactants of your systim,

Answer 5

how do i draw a possible potential energy diagram of the reaction.

Answer 6

@abb0t