Question

Holly’s camp stove uses butane (C4H10). This fuel combusts in the presence of oxygen and forms water vapor and carbon dioxide as products. The enthalpy of this reaction is –2877.5 kJ per mole. Write the correct thermochemical equation for this reaction. What does this equation tell us about the reaction? How is a thermochemical equation different from other chemical equations?

Please help me! It is urgent!!

Answer 1

The thermochemical equation for the combustion of butane is:

C₄H₁₀(g) + 6.5 O₂(g) ⇒ 4 CO₂(g) + 5 H₂O(g)   ΔH = -2877.5 kJ

It informs us of the entalphy of the reaction and it includes the states of aggregation.

What is a thermochemical equation?

A thermochemical equation is a balanced stoichiometric chemical equation that includes the enthalpy change, ΔH.

• Step 1: Write the balanced equation for the complete combustion of butane.

C₄H₁₀ + 6.5 O₂ ⇒ 4 CO₂ + 5 H₂O

• Step 2: Write the thermochemical equation.

To the previous equation, we will add the enthalpy change and the states of agregation.

C₄H₁₀(g) + 6.5 O₂(g) ⇒ 4 CO₂(g) + 5 H₂O(g)   ΔH = -2877.5 kJ

The thermochemical equation for the combustion of butane is:

C₄H₁₀(g) + 6.5 O₂(g) ⇒ 4 CO₂(g) + 5 H₂O(g)   ΔH = -2877.5 kJ

It informs us of the entalphy of the reaction and it includes the states of aggregation.

Learn more about thermochemical equations here: https://brainly.com/question/16097779