Use the values of of ∆G°f in Appendix B to calculate the stan-dar...

Question

Use the values of of ∆G°f in Appendix B to calculate the stan-dard free-energy change for the synthesis of dichloroethane from ethylene and chlorine:
C2H41g2 + Cl21g2S CH2ClCH2Cl1l2
Is it possible to synthesize dichloroethane from gaseous C2H4 and Cl2, each at 25 °C and 1 atm pressure?

Accepted Answer

Hello everyone today. We have the following problem. Using the following gibbs free energy values. To calculate or use the following gibbs free energy values To calculate the gibbs free energy change for the oxidation of a settled to hide by oxygen. So the first thing you wanna do is you wanna find our formula for the gifts for energy for the reaction. So it gives for energy for the reaction is going to be the sum of the gibbs. Free energy change of our products minus the sum of the change of our gifts for energy for our reactant. Following this we're going to take our products here or our singular product here which is acetic acid or acetic acid. We have two moles. So we're gonna take those two moles and we're gonna multiply it by that Gibbs. Free energy for acetic acid which is negative 3 kg joules per mole. That is the only product. So we're gonna bracket there and then we're gonna subtract it by the sum of our gibbs. Free energy for our reactant. So reactions We have our a Seattle to hide right there. We have two of those. So we're gonna do two times. That gives free energy change of that. The formation of that which is negative 133 kg primal. And then we're gonna add that to the one mole that we have of our oxygen and oxygen is zero kg per mole. When we get our final calculation, we're going to get the Gibbs free energy of the reaction is going to be equal to negative 514 killer jewels. And so we have to determine if the reaction is spontaneous at one atmospheres and to 98.15 kelvin. So those are known as standard state values. So if we have the standard Gibbs free energy change, which is negative 5, 14 kill jules, we have to determine if it is going to be non spontaneous or spontaneous. So since it is negative, so a negative gibbs free energy of the reaction is going to denote that this reaction is indeed spontaneous. If it were positive, it would be non spontaneous. So we can say that, yes, this reaction is spontaneous and with that we've answered the question overall, I hope this helped. And until next time.

Use the values of of ∆G°f in Appendix B to calculate the stan-dard free-energy change for the synthesis of dichloroethane from ethylene and chlorine: C2H41g2 + Cl21g2S CH2ClCH2Cl1l2 Is it possible to synthesize dichloroethane from gaseous C2H4 and Cl2, each at 25 °C and 1 atm pressure?

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