A hydrocarbon CxHy undergoes complete combustion in 100 ext cm3 of excess oxygen. After combustion, the gaseous mixture occupied 70 ext cm3. What are the values of x and y?

Step 1: Write the general balanced chemical equation for the complete combustion of a hydrocarbon C_xH_y. Assuming water produced is in liquid form at room temperature and pressure (negligible volume as a gas): C_xH_y(g) + (x + y/4)O₂(g) → xCO₂(g) + y/2H₂O(l) Step 2: Determine the volume of carbon dioxide (CO₂) produced. The gaseous mixture after combustion occupied 70 cm³. This mixture consists of CO₂ and unreacted O₂. When this mixture was passed through

A hydrocarbon CxHy undergoes complete combustion in 100 ext cm3 of excess oxygen. After combustion, the gaseous mixture occupied 70 ext cm3. What are the values of x and y?

Step 1: Write the general balanced chemical equation for the complete combustion of a hydrocarbon C_xH_y. Assuming water produced is in liquid form at room temperature and pressure (negligible volume as a gas): C_xH_y(g) + (x + y/4)O₂(g) → xCO₂(g) + y/2H₂O(l) Step 2: Determine the volume of carbon dioxide (CO₂) produced. The gaseous mixture after combustion occupied 70 cm³. This mixture consists of CO₂ and unreacted O₂. When this mixture was passed through

Solved: A hydrocarbon CxHy undergoes complete combustion in…

Write the general balanced chemical equation for the complete combustion of a hydrocarbon $C_xH_y$ .
Assuming water produced is in liquid form at room temperature and pressure (negligible volume as a gas):
$C_xH_y(g) + \left(x + \frac{y}{4}\right)O_2(g) \rightarrow xCO_2(g) + \frac{y}{2}H_2O(l)$
Determine the volume of carbon dioxide ( $CO_2$ ) produced.
The gaseous mixture after combustion occupied $70 \text{ cm}^3$ . This mixture consists of $CO_2$ and unreacted $O_2$ .
When this mixture was passed through

A hydrocarbon CxHy undergoes complete combustion in 100 ext cm3 of excess oxygen. After combustion, the gaseous mixture occupied 70 ext cm3. What are the values of x and y?

Step-by-step solution

Write the general balanced chemical equation for the complete combustion of a hydrocarbon $C_xH_y$ .

Determine the volume of carbon dioxide ( $CO_2$ ) produced.

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A hydrocarbon CxHy undergoes complete combustion in 100 ext cm3 of excess oxygen. After combustion, the gaseous mixture occupied 70 ext cm3. What are the values of x and y?

Step-by-step solution

Write the general balanced chemical equation for the complete combustion of a hydrocarbon CxHyC_xH_yCx​Hy​.

Determine the volume of carbon dioxide (CO2CO_2CO2​) produced.

Still stuck on this one?

More Chemistry Questions

Write the general balanced chemical equation for the complete combustion of a hydrocarbon $C_xH_y$ .

Determine the volume of carbon dioxide ( $CO_2$ ) produced.