Consider the following intermediate chemical equations.
CH₂(g) → C(s) + 2H₂(g)
ΔΗ, = 74.6KJ
CCl4(g) →C(s) + 2Cl₂(g)
AH₂ = 95.7 kJ
H₂(g) + Cl₂(g) → 2HCl(g)
AH₂=-92.3 KJ
What is the enthalpy of the overall chemical reaction CH4(g)+4Cl₂(g) → CCl4(g) + 4HCI(g)?
O-205.7 kJ
O-113.4 kJ
O-14.3 kJ
O 78.0 kJ

A chemical reaction can be defined as a chemical process that involves the continuous transformation (rearrangement) of the ionic, atomic or molecular structure of a chemical element by breaking down and forming chemical bonds, in order to produce a new chemical compound while new bonds are formed.

What is a chemical equation?

A chemical equation can be defined as a group of chemical symbols that is typically used in chemistry to represent the chemical reaction between two (2) or more chemical elements.

Mathematically, an expression for enthalpy of the overall chemical reaction is given by:

ΔHrxn = (n × ΔH₃) + (-n × ΔH₁) + (n × ΔH₂)

Where:

n represents the number of moles.

Substituting the given points into the formula, we have;

ΔHrxn = (2 × ΔH₃) + (-1 × ΔH₁) + (1 × ΔH₂)

ΔHrxn = (2 × (-92.3)) + (-1 × (-74.6)) + (1 × (-95.7))

ΔHrxn = -184.6 + 74.6 + 95.7

ΔHrxn = -14.3 kJ.

Read more on enthalpy here: https://brainly.com/question/12993630

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