ThermochemistryHard

Question

Use the following data to calculate the enthalpy of hydration for caesium iodide and caesium hydroxide, respectively.

Compound Lattice energy (kJ/mol) ΔHSolution (kJ/mol)

CsI +604 +33

CsOH +724 −72

Options

A.−571 kJ/mol and −796 kJ/mol
B.637 kJ/mol and 652 kJ/mol
C.−637 kJ/mol and −652 kJ/mol
D.571 kJ/mol and 796 kJ/mol

Solution

$\Delta_{\text{Lattice}}H + \Delta_{\text{Hydration}}H = \Delta_{\text{solution}}H$

$\text{For }CSl:\Delta_{\text{Hyd}}H = 33 - 604 = - 571\text{ kJ} $$$\text{For }CsOH:\Delta_{\text{Hyd}}H = ( - 72) - 724 = - 796\text{ kJ}$$

Create a free account to view solution

View Solution Free
Topic: Thermochemistry·Practice all Thermochemistry questions

More Thermochemistry Questions

For a specific work, on an average a person requires 5616 kJ of energy. How many kilograms of glucose must be consumed i...Consider the following reactions : C (s) + O2 (g) → CO2 (g) + x kJ CO (g) + O2 (g) → CO2 (g) + y kJThe heat ...Calculate the enthalpy of formation of I2O5(s) from the following data.(i) I2O5(s) + H2O(l) → 2HIO3(aq): ΔH = +4.0 kJ(ii...Oxidising power of chlorine in aqueous solution can be determined by the parameters indicated below: The energy involved...The standard enthalpy of combustion of solid boron is numerically equal to...