What is the enthalpy change for the hydration of anhydrous copper sulphate?

The enthalpy of solution of anhydrous copper sulphate (CuSO4) and hydrated copper sulphate (CuSO4. 5H2O) are – 66.5 and +11.7kJmol-1respectively.

What is Hess’s law and why enthalpy of hydration of anhydrous copper sulphate Cannot be measured directly?

This Hess’s law is used to work out the enthalpy change to form a hydrated salt from an anhydrous salt. This cannot be done experimentally because it is impossible to add the exact amount of water to hydrate the copper salt and it is not easy to measure the temperature change of a solid turning into another solid.

What is the magnitude of enthalpy of solution of anhydrous copper II sulphate in kJ mol?

-66.5 kJ/mol
Given that the enthalpy of solution of the hydrated copper (II) sulphate is +11.3 kJ/mol, what is the enthalpy of hydration of the anhydrous solid? (Enthalpy of solution of anhydrous copper (II) sulphate is -66.5 kJ/mol).

Why it is difficult to measure the enthalpy change directly when an anhydrous salt is converted to a hydrated salt?

It is difficult to measure the enthalpy change directly when an anhydrous salt is converted to a hydrated salt, because we can not add the exact amount of water to hydrate the anhydrous salt and it is difficult to measure the temperature change of a solid turning into another solid.

What is the enthalpy of CuSO4?

The enthalpy of solution of anhydrous CuSO4 is – 16 kcal and that of CuSO4.

Why is it not possible to measure the enthalpy change of decomposition directly?

The reaction takes place at high temperature and requires heating. The enthalpy change can not be measured directly because you have to take into account how much energy was put into the reaction in the first place.

What is the magnitude of enthalpy of solution of anhydrous copper?

What is the molar heat of solution of anhydrous copper II sulphate?

– 15.9 kcal
The heat of solution of anhydrous CuSO4 is – 15.9 kcal and that of CuSO4. 5H2O is 2.8 kcal .

How do you measure enthalpy change in copper sulfate?

Measurement of an enthalpy change To determine an enthalpy change which cannot be measured directly. The reaction involves the conversion of anhydrous copper (II) sulfate into hydrated copper (II) sulfate. 0 º C to 50 °C glass or digital thermometer (0.1°C or 2°C divisions are desirable but not essential)

How to prepare anhydrous copper(II) sulfate solution?

At the fourth minute, add the powdered anhydrous copper (II) sulfate rapidly to the water in the polystyrene cup and continue to stir, but do not record the temperature. At the fifth minute and for every minute up to fifteen minutes, stir and record the temperature of the solution in the polystyrene

How much hydrated copper (II) sulfate should I weigh?

Weigh out between 20g and 6.30g of hydrated copper (II) sulfate in a dry stoppered weighing bottle. The precise mass should be recorded. Construct a suitable Table of results to allow you to record temperatures at minute intervals up to 15 minutes as you did for Experiment 1.

What is Hess’s law in chemistry?

1 N Goalby chemrevise.org 3.12 Hess’s Law. Hess’s law states that total enthalpy change for a reaction is independent of the route by which the chemical change takes place. Hess’s law is a version of the first law of thermodynamics, which is that energy is always conserved. 2H (g) + 2Cl(g) H2 + Cl 2.