Question

When C2H5Cl(g) is burned in oxygen, chlorine gas is produced in addition to carbon dioxide and water vapor. 5145 kJ of heat are released for every four moles of C2H5Cl(g) burned. Which of the following correctly represents the thermochemical equation?

Answer 1

Answer: The chemical equation is written below.

Explanation:

Combustion reaction is defined as the chemical reaction in which a hydrocarbon reacts with oxygen gas to produce carbon dioxide gas and water molecule.

$\text{hydrocarbon}+O_2\rightarrow CO_2+H_2O$

The chemical equation for the combustion of ethyl chloride follows:

$4C_2H_5Cl+13O_2\rightarrow 2Cl_2+8CO_2+10H_2O$

We are given:

When 4 moles of ethyl chloride is burnt, 5145 kJ of heat is released.

For an endothermic reaction, heat is getting absorbed during a chemical reaction and is written on the reactant side.

$A+\text{heat}\rightleftharpoons B$

For an exothermic reaction, heat is getting released during a chemical reaction and is written on the product side

$A\rightleftharpoons B+\text{heat}$

So, the chemical equation follows:

$4C_2H_5Cl+13O_2\rightarrow 2Cl_2+8CO_2+10H_2O+5145kJ$

Hence, the chemical equation is written above.