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ICSE Class 10 Chemistry Question 1 of 37

Mole Concept and Stoichiometry — Question 7

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Question

Question 6

What volume of oxygen at STP is required to affect the combustion of 11 litres of ethylene [C2H4] at 273°C and 380 mm of Hg pressure?

C2H4 + 3O2 ⟶ 2CO2 + 2H2O

Answer

C2H4+3O2⟶2CO2+2H2O1 vol.:3 vol.11 lit:33 lit\begin{matrix} \text{C}_2\text{H}_4 & + & 3\text{O}_2 & \longrightarrow & 2\text{CO}_2 + 2\text{H}_2\text{O} \\ 1 \text{ vol.} & : & 3 \text{ vol.} \\ 11 \text{ lit} & : & 33 \text{ lit} \end{matrix}

STPGiven Values
P1 = 760 mm of HgP2 = 380 mm of Hg
V1 = x litV2 = 33 lit
T1 = 273 KT2 = 273 + 273 K = 546 K

Using the gas equation,

P1V1T1=P2V2T2\dfrac{P_{1}V_{1}}{T_{1}} = \dfrac{P_{2}V_{2}}{T_{2}}

Substituting the values we get,

760×x273=380×33546x=380×33×273546×760x=3,423,420414,960x=8.25 lit\dfrac{760 \times x}{273} = \dfrac{380 \times 33}{546} \\[0.5em] x = \dfrac{380 \times 33 \times 273}{546 \times 760 } \\[0.5em] x = \dfrac{3,423,420}{414,960} \\ \\[0.5em] x = 8.25 \text{ lit}

Hence, volume of oxygen required = 8.25 lit.