Which of the following indicates a reaction with a positive ΔG? A. endergonic, spontaneous B. endergonic, not spontaneous C. exergonic, spontaneous D. exergonic, not spontaneous

B. endergonic, not spontaneous

Explanation:

Endergonic reactions are defined as the reactions in which energy of the product is greater than the energy of the reactants. The total energy is absorbed in the form of heat and   for the reaction comes out to be positive.

The Gibbs equation is:

= Gibb's free energy change

= enthalpy change

T = temperature

= entropy change

A reaction is non spontaneous when = Gibb's free energy change is positive

Thus the reaction has to be endergonic.

the answer would be c

answer: the value of enthalpy change will be -152.80 kj.

solution:

pressure = 1atm , temperature = = 298 k

given that pressure and temperature are same in both gases , the number of moles of both gases can be determined by the ideal gas equation.

according to reaction 3 moles no are reacting with 1 mol of ,then 0.49 mol of no will react with moles of ozone that is 0.16 moles of ozone. since, no is limiting reagent and is an excessive reagent.

enthalpy change for the reaction between the given volumes of the gases is :