N2 and O2 gases react to form dinitrogen pentoxide(N2O5).Calculate deltaH and deltaU for this process per mol of N2 gase knowing that when 101.7g of N2 react with 102.97g of O2 at 25DegC and a constant pressure of 1 atm, 533.5kJ of energy is released as heat.
2N2g + 5O2g-----2N2O5g
help thank you
To calculate the enthalpy change (ΔH) and internal energy change (ΔU) for the reaction of N2 and O2 gases to form N2O5, you will need to use the concept of Hess's law and the given information on energy released.
Hess's law states that the total enthalpy change for a reaction is independent of the pathway taken. In other words, the overall enthalpy change is the sum of the enthalpy changes of individual steps of a reaction.
Let's begin by calculating the enthalpy change (ΔH) for the given reaction:
2N2(g) + 5O2(g) --> 2N2O5(g)
Given energy released as heat = -533.5 kJ
To calculate ΔH, we can use the equation:
ΔH = ΣΔH(products) - ΣΔH(reactants)
Now, we need to find the enthalpy changes for the reactants and products. These values can be found in the standard enthalpy of formation (ΔHf) tables.
The reaction equation shows that 2 moles of N2O5 are formed. We need to multiply the ΔHf of N2O5 by 2.
ΔH(products) = 2 ΔHf(N2O5)
Next, we can do the same for the reactants:
ΔH(reactants) = ΔHf(N2) + 5 ΔHf(O2)
Now we can substitute these values into the equation to find ΔH:
ΔH = 2 ΔHf(N2O5) - (ΔHf(N2) + 5 ΔHf(O2))
To calculate ΔH, you will need to look up the values for the standard enthalpy of formation (ΔHf) of N2(g), O2(g), and N2O5(g) from reference sources (such as textbooks or online databases).
Once you have these values, substitute them into the equation above and calculate ΔH.
To calculate the internal energy change (ΔU) for the reaction, you can use the equation:
ΔU = ΔH - ΔPV
Where ΔP is the change in pressure and ΔV is the change in volume. However, since the given information states that the reaction is carried out at a constant pressure of 1 atm, ΔP can be assumed to be 0. Therefore, the equation simplifies to:
ΔU = ΔH
Therefore, in this case, ΔU is equal to ΔH.
Remember to double-check the values and unit conversions of the enthalpy values to ensure accurate calculation.