Saved Bookmarks
| 1. |
If the enthalpy of vaporisation of water is `186.5 J mol^(-1)`, then entropy of its vaporisation will beA. `4.0 JK^(-1)mol^(-1)`B. `3.0JK^(-1) mol^(-1)`C. `1.5JK^(-1) mol^(-1)`D. `0.5 JK^(-1)mol^(-1)` |
|
Answer» Correct Answer - A ` Delta _("vap") H = 186.5 J//mol = 0.1865 KJ//mol.` Temperature T = ` 273 + 100 = 373 K ` ` Delta _("vap") H^(@) = 0.1865 KJ//mol` Entropy changes `Delta S = (Delta_("vap").H^(@))/T` ` T = 273 + 100 = 373 K` ` = (0.1865)/373 = 0.5J//K mol` |
|