ThermochemistryMedium
Question
The value of ΔHsol of anhydrous copper (II) sulphate is −66.11 kJ. Dissolution of 1 mole of blue vitriol, [Copper (II) sulphate pentahydrate] is followed by the absorption of 11.5 kJ of heat. The enthalpy of dehydration of blue vitriol is
Options
A.−77.61 kJ
B.+77.61 kJ
C.−54.61 kJ
D.+54.61 kJ
Solution
Given T.C.E. are
(a) $CuSO_{4}(s) + aq \rightarrow CuSO_{4}(aq);\Delta H = - 66.11\text{ kJ}$
(b) $CuSO_{4}.5H_{2}O(s) + aq \rightarrow CuSO_{4}(aq);\Delta H = + 11.5\text{ kJ}$
Required T.C.E. is
$CuSO_{4}.5H_{2}O(s) \rightarrow CuSO_{4}(s);\Delta H = ? $$$\text{From }(b) - (a);\Delta H = 11.5 - ( - 66.11) = 77.61\text{ kJ}$$
Create a free account to view solution
View Solution FreeMore Thermochemistry Questions
Enthalpies of combustion of CH4, C2H6 and C3H8 are −210, −370 and −526 kcal/mol, respectively. Enthalpy of combustion of...For which of the following substance(s), the standard enthalpy of formation is/are zero?...The enthalpy change for a reaction does not depend upon...The heat of combustion of yellow phosphorous is - 9.91 kJ and of red phosphorous to redphosphorus is :...The bond energies (in kJ/mol) at 25°C are C–C = 346, C–H = 413, H–H = 437, C = C; 611. From these data, the value of ΔH ...