ThermochemistryHard

Question

Heat absorbed in the reaction H2(g) + Cl2(g) → 2HCl(g) is 182 kJ. Bond energies of H–H = 430 kJ/mole and Cl–Cl = 242 kJ/mole. The H–Cl bond energy is

Options

A.763 kJ/mole
B.245 kJ/mole
C.336 kJ/mole
D.154 kJ/mole

Solution

$+ 182 = (430 + 242) - \left( 2 \times B.E._{H - Cl} \right)$

$\therefore B.E._{H - Cl} = 245\text{ kJ/mol}$

Create a free account to view solution

View Solution Free
Topic: Thermochemistry·Practice all Thermochemistry questions

More Thermochemistry Questions

Equal volumes of one molar hydrochloric acid and one molar sulphuric acid are neutralized completely by dilute NaOH solu...The data below refers to gas phase reaction at constant pressure at 25°C.CH3–CH3 → CH3–CH2 + H: ΔH1 = +420 kJ mol–1CH3–C...A quantity that cannot be directly measured is...Among the following the reaction for which ΔH = ΔE is...The enthalpy of atomization of PH3(g) is +954 kJ/ mol and that of P2H4 is +1.488 MJ/mol. The bond energy of the P–P bond...