The volume of 2 mol hydrogen gas at 1 atm pressure and 273 K is 44.8 L.
a) Name the scientist who established the relationship between the volume and pressure of a gas through experiment.
b) What will be the new pressure ifthe volume of hydrogen gas is changed to 22.4 L.
[Hint: Temperature is constant]
c) Suggest a method to increase the volume of this gas without changing the pressure and mass.
Answers
Explanation:
Given: Mass of elemental boron = 21.6 g
Temperature = 273 K
Pressure = 1 atm
Solution: The balanced chemical equation for the reduction of boron dichloride is
BCl
3
+1.5H
2
→B+3HCl
From the equation, it is clear that 1 mole of boron formation requires 1.5 moles of hydrogen gas.
Let's calculate the moles of boron from the given mass of boron.
No. of moles =
Molar mass
Mass
=
10.8 gmol
−1
21.6g
= 2.00 mol
So, to obtain 2.00 mol of boron, 3.00 mol of hydrogen gas is required.
One mole of hydrogen gas at 273 K and 1 atm occupies a volume of 22.4L.
Therefore, volume of hydrogen gas = 3.00mol×22.4 Lmol
−1
= 67.2L