Question

the volume occupied by 4g of gas at 1 atm and 273k if its vapour density is 30 is?​

Answer 1

Answer:

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

$BCl </p><p>3</p><p> </p><p> +1.5H </p><p>2</p><p> </p><p> →B+3HCl$

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.

$No. of moles = \frac{Molar mass }{Mass} </p><p></p><p>$

$\frac{21.6g}{10.8g \: mole {}^{ - 1} } </p><p> </p><p> </p><p> </p><p> </p><p> = 2.00 mol$

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