What is the chemical equation that corresponds to the standard molar enthalpy of formation of N2O?
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The chemical equation that corresponds to the standard molar enthalpy of formation of N2O is:
N2(g) + O2(g) → 2NO(g)
The standard molar enthalpy of formation (∆Hf) of N2O is the enthalpy change when one mole of N2O is formed from its elements in their standard states (N2 and O2), at a constant pressure of 1 atmosphere and a specified temperature (usually 298 K).
To find the chemical equation that corresponds to the standard molar enthalpy of formation of N2O, you can use thermodynamic data and Hess's Law.
The standard molar enthalpy of formation (ΔHf) is defined as the change in enthalpy when one mole of a compound is formed from its constituent elements in their standard states at a given temperature and pressure.
The standard molar enthalpy of formation of N2O can be determined by considering the balanced chemical equation representing the formation of N2O from its constituent elements.
From the periodic table, we find that the standard states of nitrogen (N2) and oxygen (O2) are diatomic gases. The standard state for nitrogen dioxide (NO2) is a gas as well.
First, we need to write the balanced equation for the formation of N2O:
N2(g) + O2(g) → N2O(g)
However, the reaction above does not perfectly represent the formation since oxygen gas (O2) is not the standard state for oxygen.
To correct this, we can use the following equation:
2NO2(g) → N2O(g) + O2(g)
Now, we can use Hess's Law to calculate the standard molar enthalpy of formation of N2O.
Hess's Law states that if a reaction can be expressed as the sum of two or more other reactions, the change in enthalpy for the overall reaction is also the sum of the enthalpy changes of the individual reactions.
We need to refer to the standard enthalpy changes of the reactions involved:
N2(g) + O2(g) → 2NO2(g) ΔH1
2NO2(g) → N2O(g) + O2(g) ΔH2
By understanding that the enthalpy change for the reverse reaction is equal in magnitude but opposite in sign, we can rewrite the equations as follows:
ΔH1 = -ΔHf[N2O] - [ΔHf[O2] (1)
ΔH2 = -ΔHf[N2O] - ΔHf[O2] (2)
Now, we need to solve for ΔHf[N2O].
By subtracting equation (2) from equation (1), we get:
ΔH1 - ΔH2 = ΔHf[O2]
Substituting the given standard enthalpy changes, we find:
0 = -ΔHf[N2O] - 0.5 * ΔHf[O2]
Simplifying the equation:
ΔHf[N2O] = - 0.5 * ΔHf[O2]
Therefore, the chemical equation that corresponds to the standard molar enthalpy of formation of N2O is:
N2(g) + 0.5O2(g) → N2O(g)
Please note that the standard molar enthalpy of formation values for N2O and O2 need to be known to calculate the enthalpy of formation for N2O accurately.