Answer: The molarity of this solution is 0.159 M.
Explanation:
Given: Mass of solute = 16.3 g
Volume = 1.75 L
Number of moles is defined as the mass of substance divided by its molar mass.
Hence, moles of NaCl (molar mass = 58.44 g/mol) ar calculated as follows.

Molarity is the number of moles of a substance present in a liter of solution.
So, molarity of the given solution is calculated as follows.

Thus, we can conclude that the molarity of this solution is 0.159 M.
No. The answer is false.
Just read that sentence aloud and you'll know that it does not sound right
A 3.1 L sample of hydrogen <u>d. contains the same number of molecules</u>
as 3.1 L of carbon dioxide at the same temperature and pressure.
This is the fundamental principle of <em>Avogadro’s hypothesis</em>: equal volume of gases at the same temperature and pressure contain the same number of molecules.
The sample of carbon dioxide has a <em>greater mass</em>, a <em>greater number of atoms</em>, and a <em>greater density</em>, than the sample of hydrogen.
H₂ is the limiting reactant.
<u>Explanation:</u>
H₂ reacts with O₂
The reaction would be
2H₂ + O₂ → 2H₂O
According to the balanced equation, 2 moles of H₂ reacts with 1 mole of O₂ to form 2 moles of H₂O.
The ratio of usage of H₂ and O₂ is 2 : 1 respectively
If 3 moles of H₂ and 2 moles of O₂ are present then:
3 moles of H₂ would require 1.5 moles of O₂ ( 2 : 1 of H₂ and O₂ )
Out of 2 moles of O₂, 1.5 moles would be used and 0.5 mole would be in excess.
Therefore, H₂ is the limiting reactant as the number of moles of H₂ are not enough to use all the O₂.