Ethyl alcohol has ΔHfusion = 5.02 kJmol and melts at - 114.1 °C....

Question

Ethyl alcohol has ΔHfusion = 5.02 kJ>mol and melts at - 114.1 °C. What is the value of ΔSfusion for ethyl alcohol?

Accepted Answer

Hello everyone today. We have the following problem, Naphthalene has a melting point of 80.3°C, calculate the entropy change of fusion for naphthalene. And then we have the value for the entropy change here which is 19.2 kg joules per mole. So the first thing that we want to recall is our gibbs free energy equation which is the gibbs free energy is equal to our entropy change minus the temperature times The entropy change. We also want to change our degrees from Celsius to kelvin. So we're simply gonna add to 73.15 to get 353.45 Kelvin. Now that we have this we can go ahead and solve our problem. So what is gonna be our gifts for energy? So at the melting point? So at melting point RK value is going to equal one and the energy of fusion is going to equal zero. Therefore we can substitute zero for our gibbs free energy Moreover, our entropy of fusion was said to be 19.2 kg primal. We're gonna subtract this from our temperature that we found which was .45 Kelvin. And then we're gonna multiply by our unknown variable, Solving for the unknown variable. We're going to get that our entropy change is going to be equal to 19. kg joules per mole times and we're going to have to transform this from killer jewels, two jewels. We're gonna use our conversion factor that one kg joule is equal to 10 to the third jewels. And then we're going to divide all of this by our temperature of 53.45 kelvin. When our units cancel out, we will result in an entropy change of 54. jewels per mole kelvin as our final answer. And with that we have solved the problem Overall, I hope this helped until next time.

Ethyl alcohol has ΔHfusion = 5.02 kJ>mol and melts at - 114.1 °C. What is the value of ΔSfusion for ethyl alcohol?

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