Bright Tutorials Bright Tutorials
ICSE Class 10 Chemistry Question 26 of 72

Mole Concept & Stoichiometry Miscellaneous Exercises — Question 26

Back to all questions
26
Question

Question 25

Hydrogen sulphide gas burns in oxygen to yield 12.8 g of sulphur dioxide gas as under:

2H2S + 3O2 ⟶ 2H2O + 2SO2

Calculate the volume of hydrogen sulphide at S.T.P. Also, calculate the volume of oxygen required at S.T.P. which will complete the combustion of hydrogen sulphide determined in (litres).

Answer

2H2S+3O2⟶2H2O+2SO22 Vol.3 Vol.2 Vol.2[2(1)+32]3[2(16)]2[32+2(16)]68 g96 g128 g\begin{matrix} 2\text{H}_2\text{S} & + &3\text{O}_2 & \longrightarrow & 2\text{H}_2\text{O} & + & 2\text{SO}_2 \\ 2\text{ Vol.} && 3\text{ Vol.} && && 2\text{ Vol.} \\ 2[2(1) + 32] && 3[2(16)] &&&& 2[32 + 2(16)] \\ 68 \text{ g} && 96 \text{ g} &&&& 128 \text{ g} \end{matrix}

128 g of SO2 has volume 2 × 22.4 litres

∴ 12.8 g of SO2 has volume =

2×22.4128\dfrac{2 × 22.4}{128} x 12.8 = 4.48 L

Volume of oxygen = ?

2 × 22.4 L H2S requires = 3 × 22.4 litre of oxygen

∴ 4.48 L H2S will require

3×22.42×22.4\dfrac{3 × 22.4}{2 × 22.4 } x 4.48 = 6.72 L of oxygen.