What volume of Hydrogen gas, at $273$ K and $1$ atm pressure will be consumed in obtaining $21.6$ g of elemental boron?
(Atomic mass = $10.8$ ) from the reduction of boron chloride by hydrogen.)

22.4

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89.6

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67.2

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44.8

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Solution

The correct option is C $67.2$ l
$2 B C l_{3} + 3 H_{2} ⟶ 2 B + 6 H C l$
$\Rightarrow 2 \times 10.8 g$ Boron= $3 \times 22.42 H_{2}$
$∴ 21.6 g$ Boron= $\frac{3 \times 22.4 \times 2.16}{2 \times 10.8}$
$\Rightarrow 67.2 L$

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Similar questions

What volume of hydrogen gas at 273 K and 1 atm pressure will be consumed to obtain 21.6 g of elemental boron (atomic mass = 10.8) from the reduction of boron trichloride by hydrogen?

Q. What volume of hydrogen gas, at 273 K and 1 atm pressure will be consumed in obtaining 21.6 g of elemental boron (atomic mass 10.8) from reduction of boron trichloride by hydrogen?

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Q. What volume of hydrogen gas (in litres) at 273 K and 1 atm pressure will be consumed to obtain 21.6 g of elemental boron (atomic mass = 10.8) from the reduction of boron trichloride by hydrogen?

Q. The volume (in litres) of hydrogen gas at

273

K and

1

atm pressure that will be consumed in obtaining

21.6

g of elemental boron (atomic mass

= 10.8

amu) from reduction of boron trichloride by hydrogen gas is : (as nearest integer)

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What volume of Hydrogen gas, at 273K and 1 atm pressure will be consumed in obtaining 21.6 g of elemental boron? (Atomic mass = 10.8) from the reduction of boron chloride by hydrogen.)

The correct option is C 67.2l2BCl3+3H2⟶2B+6HCl⇒2×10.8g Boron= 3×22.42H2∴21.6g Boron= 3×22.4×2.162×10.8⇒67.2L

What volume of Hydrogen gas, at $273$ K and $1$ atm pressure will be consumed in obtaining $21.6$ g of elemental boron?
(Atomic mass = $10.8$ ) from the reduction of boron chloride by hydrogen.)

The correct option is C $67.2$ l
$2 B C l_{3} + 3 H_{2} ⟶ 2 B + 6 H C l$
$\Rightarrow 2 \times 10.8 g$ Boron= $3 \times 22.42 H_{2}$
$∴ 21.6 g$ Boron= $\frac{3 \times 22.4 \times 2.16}{2 \times 10.8}$
$\Rightarrow 67.2 L$