An unknown compound has the empirical formula CH2O and a molecular mass of 180 amu. What is the molecular formula of the compoun
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The standard enthalpy of formation (Δ) is a measure of the energy released or consumed when one mole of a substance is created under standard conditions from its pure elements.
Standard enthalpies (Δ) of formation for given reaction is 978.3 kJ
The standard enthalpy of formation is defined as the enthalpy change when one mole of a substance in the standard state (1 atm of pressure and 298.15 K) is formed from its pure elements under the same conditions.
Given reaction ;
To Find : Δ
Δ = ∑np Δ
(products) – ∑np Δ
(reactants)
Δ = [1(Δ
) + 4(Δ
)] – [1(Δ
) + 4(Δ
)]
Δ = [1(0) + 4(-241.8)] – [1(+9.16) + 4(0)]
Δ = [4(-241.8)] – [1(+9.16)] = 978.3 kJ
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