400 ml of a sample of coal gas containing 40% H 2 ( g ) , 35% CH 4 ( g ) , 15% CO ( g ) and 10% C 2 H 2 ( g ) was mixed with 2500 ml of air containing 20% oxygen by volume and exploded and res

Question

400 ml of a sample of coal gas containing 40% H 2 ​ ( g ) , 35% CH 4 ​ ( g ) , 15% CO ( g ) and 10% C 2 ​ H 2 ​ ( g ) was mixed with 2500 ml of air containing 20% oxygen by volume and exploded and resulting solution is cooled. Then after explosion.

TestHub · Accepted Answer

Question Explanation: Calculating final mixture volume after combustion of coal gas.

Concept: Stoichiometry.

Solution: First, calculate the initial volumes of all reactive gases in the coal gas and the volume of $O_{2}$ in the air. Then, use the balanced combustion equations for each component ( $H_{2}, CH_{4}, CO, C_{2} H_{2})$ to find the total $O_{2}$ consumed and total $CO_{2}$ produced. The final volume is the sum of $CO_{2}$ , unreacted $O_{2}$ , and inert $N_{2}$ .

$(1, 4)$

So Total $VO_{2}$ used $= 80 + 280 + 30 + 100 = 490 ml$

$VO_{2}$ left $\500 - 490 = 10 ml$

$VCO_{2}$ produced $= 140 + 60 + 80 = 280 ml$

$∴ V_{f} = VCO_{2} + (VO_{2})_{left} + V_{air}$

$= 280 + 10 + 2000 ml = 2290 ml$

Final Answer: Statements 1 and 4 are correct.

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