For the following questions, use the reaction NO2(g) - 1/2 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

please no fake answers I worked hard to get these points :/

the ideal gas law equation is as follows

pv = nrt

where p - pressure

v - volume

n - number of moles

r - universal gas constant

t - temperature

so if the pressure, volume and temperature are already known

we are left with n and r

since r is the universal gas constant that has a known fixed value then r too is known

so we are left with 'n'

once we know temperature volume and pressure

we can find the number of moles of gas present using the ideal gas law equation

this is not my own answer, this is an answer for the same question by the user blahblahmali. i do not claim ownership of this account.