# calculate the approximate enthalpy change , δh∘, for the combustion of methane:

**How do you calculate the enthalpy of combustion of methane?** – So the standard enthalpy of combustion of methane is equal to minus minus 74.6 plus minus 393.51 plus two times minus 285.83. Which is equal to 74.6 minus 393.51 minus 571.66, which is equal to minus 890.57 kilojoules per mole.

**How do you calculate the enthalpy of enthalpy of combustion?** –

**How do you calculate the standard enthalpy change of formation of methane?** –

**What is the value of ΔH δ H for the combustion of one mole of methane?** – The combustion of methane, CH4, releases 890.4 kJ/mol. That is, when one mole of methane is burned, 890.4 kJ are given off to the surroundings. This means that the products have 890.4 kJ less than the reactants. Thus, AH for the reaction = – 890.4 kJ.

**What is enthalpy of methane?** – Hence the enthalpy of formation of methane is −75kJ.

**What is the enthalpy change of combustion?** – The standard enthalpy change of combustion of a compound is the enthalpy change which occurs when one mole of the compound is burned completely in oxygen under standard conditions, and with everything in its standard state.

**How do you calculate enthalpy of combustion using Hess’s law?** –

**How do you calculate enthalpy change?** – Use the formula ∆H = m x s x ∆T to solve. Once you have m, the mass of your reactants, s, the specific heat of your product, and ∆T, the temperature change from your reaction, you are prepared to find the enthalpy of reaction. Simply plug your values into the formula ∆H = m x s x ∆T and multiply to solve.