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Chapter 1: QCYL (page 9)

Hydrogen gas, H2, reacts explosively with gaseous chlorine, \({\bf{C}}{{\bf{l}}_{\bf{2}}}\), to form hydrogen chloride, HCl(g). What is the enthalpy change for the reaction of 1 mole of \({{\bf{H}}_{\bf{2}}}\)(g) with 1 mole of \({\bf{C}}{{\bf{l}}_{\bf{2}}}\)(g) if both the reactants and products are at standard state conditions? The standard enthalpy of formation of HCl(g) is 鈭�92.3 kJ/mol.

Short Answer

Expert verified

\({\rm{\Delta Hf^\circ }}\)for two moles of HCl = -184. 6 kJ/mol.

Step by step solution

01

Given reaction

The reaction of 1 mole of \({{\rm{H}}_{\rm{2}}}\)(g) with 1 mole of \({\rm{C}}{{\rm{l}}_{\rm{2}}}\)(g) is given by:

\({{\rm{H}}_{\rm{2}}}\left( {\rm{g}} \right){\rm{ + C}}{{\rm{l}}_{\rm{2}}}\left( {\rm{g}} \right) \to {\rm{2 HCl}}\left( {\rm{g}} \right){\rm{\;\;\Delta Hf^\circ = - 92}}{\rm{.3 kJ/mol}}\)

The change of enthalpy of one mole of HCl is -92.3 kJ/ mol is used to find the heat produced when one mole of HCl is formed.

02

Enthalpy change

Enthalpy change refers to the heat released inside or outside a system in a reaction.

The enthalpy change is evaluated as:

\(\begin{array}{*{20}{l}}{{\rm{\Delta Hf^\circ for one mole HCl = \;\; - 92}}{\rm{.3 kJ/mol}}}\\\begin{array}{l}{\rm{\Delta Hf^\circ for two moles of HCl\; = 2 \times 92}}{\rm{.3 }}\\{\rm{ = - 184}}{\rm{.6 kJ/mol\;\;\;\;\;\;\;\;\;\;\;\;\;\;\;\;\;\;\;\;\;\;\;\;\;\;\;\;\;}}\end{array}\end{array}\)

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Most popular questions from this chapter

The density (d) of a substance is an intensive property that is defined as the ratio of its mass(m) to its volume (V).

\(\begin{aligned}{\rm{density = }}\frac{{{\rm{mass}}}}{{{\rm{volume}}}}\\{\rm{d = }}\frac{{\rm{m}}}{{\rm{v}}}\end{aligned}\)

Considering that mass and volume are intensive properties, explain why their ratio, density is intensive.

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