18.5 grams of Nitrogen gas and 26.7 grams of Oxygen gas form how many grams of Dinitrogen Pentoxide if the reaction is only 80% efficient? ***THE PERCENTAGE DOES NOT CONTRIBUTE TO THE SIG FIGS... ONLY THE MEASURED MASSES OF THE GASES***

29.38 grams

Explanation:

The reaction is:

2N₂(g) + 5O₂(g) → 2N₂O₅    (1)

We need to calculate the number of moles of N₂ and O₂:

Now, we need to find the limiting reactant. From reaction (1) we have that 2 moles of N₂ react with 5 moles of O₂:

If we have 0.66 moles of N₂ and we need 0.34 moles to react with O₂, then the limiting is O₂.

We can calculate the number of moles of N₂O₅ produced:

Now, we can calculate the theoretical mass of N₂O₅:

Finally, if the reaction is only 80% efficient then the mass of N₂O₅  produced is:

Therefore, are formed 29.38 grams of N₂O₅.

I hope it helps you!

vanderwaal's forces of attraction are the electrostatic intermolecular forces that exist in a molecule due to the temporary or permanent dipoles that are developed in a molecule. in , the major intermolecular forces are dipole-dipole interactions as the molecule is polar (bent structure). so the vanderwaal's forces of interaction in between molecules are the permanent dipole-dipole interactions that develop due to the dipole that exists in between the polar h - s bond. the positively charged hydrogen atom is attracted towards the negative end of the dipole that is sulfur of the adjacent molecule. therefore, these forces of attraction are relatively stronger than that of london dispersion forces that exist in non polar molecules.

what does the table look like