Question

A Questic

Is the following reaction feasible at 340K? Mg + ZnO -> MgO + Zn Enthalpy Data: Mg: 0 kJ/mol ZnO: -348 kJ/mol MgO:-602
kJ/mol Zn: 0 kJ/mol Entropy Data: Mg: 33 J/K mol ZnO: 44 J/K mol MgO: 42 J/K mol Zn: 27 J/K mol
A. No, it is not feasible because the Gibbs free energy change is negative.
OB. Yes, it is feasible because the Gibbs free energy change is negative.
C. No, it is not feasible because the Gibbs free energy change is positive.
D. Yes, it is feasible because the Gibbs free energy change is positive.

Answer 1

B. Yes, it is feasible because the Gibbs free energy change is negative.

Step-by-step explanation:

I passed the exam 100/100

Answer 2

No, it is not feasible because the Gibbs free energy change is positive

Step-by-step explanation:

∆Hreaction= (-602 KJ/mol) - (-348 KJ/mol) = -254 KJ/mol

∆Sreaction = (42 + 27) J/Kmol - (33 + 44) J/K = -8J/Kmol

From;

∆G = ∆H - T∆S

∆G = 254 × 10^3 J/mol - [340K × (-8 J/Kmol)]

∆G = 2.57 × 10^5 J/mol

Note that when the change in free energy is positive, a reaction is non spontaneous. Only a reaction that has a negative change in free energy is spontaneous.