Using Hess's Law and the provided reactions, calculate the heat of formation of propane (C3H8).

May 4, 2026Chemistry

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2 stepsMay 4, 2026

Answer

-393 \text{ kJ/mol}$

Hey Arnold, good to see you again.

To determine the heat of formation of propane ( $\text{C}_3H_8$ ), we will use Hess's Law. The target equation is: $3C(s) + 4H_2(g) \longrightarrow C_3H_8\text{(g)}$

We are given the following reactions and their enthalpy changes:

$\text{C(s)} + O_2(g) \longrightarrow CO_2\text{(g)}$ ; $\Delta H_1 = -393 \text{ kJ/mol}$
$\text{H}_2\text{(

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Quick Answer

Hey Arnold, good to see you again. To determine the heat of formation of propane (C_3H_8), we will use Hess's Law.

Asked on May 4, 2026Chemistry

This chemistry question involves key chemical concepts and calculations. The detailed solution below walks through each step, from identifying the reaction type to computing the final answer.

ScanSolve AI AnswerAnswered on May 4, 2026

Hey Arnold, good to see you again. To determine the heat of formation of propane (C_3H_8), we will use Hess's Law. The target equation is: 3C(s) + 4H_2(g) C_3H_8(g) We are given the following reactions and their enthalpy changes: 1. C(s) + O_2(g) CO_2(g); H_1 = -393 kJ/mol 2. $H_2(