Enthalpy of reaction: -41.15 kJ
Entropy change: -42.36 kJ
The way to start it is simply by converting 0.239 L of dinitrogen oxide gas into moles of gas using the ideal gas equation
at STP , 1 mol of gas is 22.4 L of gas, or you could simply use pv = nRT
hope this helps
Answer: 17) d. ![C_2H_6](https://tex.z-dn.net/?f=C_2H_6)
18. c. The empirical formula of a compound can be twice the molecular formula.
Explanation:
Molecular formula is the chemical formula which depicts the actual number of atoms of each element present in the compound.
Empirical formula is the simplest chemical formula which depicts the whole number of atoms of each element present in the compound.
To calculate the molecular formula, we need to find the valency which is multiplied by each element to get the molecular formula.
The equation used to calculate the valency is:
![n=\frac{\text{molecular mass}}{\text{empirical mass}}](https://tex.z-dn.net/?f=n%3D%5Cfrac%7B%5Ctext%7Bmolecular%20mass%7D%7D%7B%5Ctext%7Bempirical%20mass%7D%7D)
The empirical mass can be calculated from empirical formula and molar mass must be known.
17. Thus the empirical formula of
should be ![CH_3](https://tex.z-dn.net/?f=CH_3)
18. The molecular formula will either be same as empirical formula or is a whole number multiple of empirical formula. Thus the empirical formula of a compound can never be twice the molecular formula.