10.0 g of gaseous ammonia and 6.50 g of oxygen gas are introduced into a previously evacuated 5.50 l vessel. if the ammonia and oxygen then react to yield no gas and water vapor, what is the final density of the gas mixture inside the vessel at 23°c?

The density is 3g/L

Explanation:

The reaction that occurs in the vessel is:

4 NH₃ + 5 O₂ → 4 NO + 6 H₂O

10,0g of NH₃ are:

6,50 g of O₂ are:

For a complete reaction of O₂ there are necessaries:

O₂ is limiting reactant. The excess moles of NH₃ are:

0,587 - 0,163 = 0,424 moles of NH₃

These moles are:

7,22g of NH₃

Knowing O₂ is limiting reactant, mass of NO and H₂O are:

4,87g of NO

4,39g of H₂O

The total mass is: 7,22g + 4,87g + 4,39g = 16,48g ≡ 16,5g

-The same mass add in the first. By matter conservation law-

As vessel volume is 5,50L, density is:

16,5g/5,50L = 3g/L

I hope it helps!

there are no statements provided but here is why:

sulfur belongs to group 16 because it can be found in nature whether it is in a free or combined state.

hope this

it is a solid

explanation: