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?

April 28, 2026Chemistry

ScanSolve AI Answer

April 28, 2026

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): $C_xH_y(g) + \left(x + \frac{y}{4}\right)O_2(g) \rightarrow xCO_2(g) + \frac{y}{2}H_2O(l)$

Step 2: Determine the volume of carbon dioxide ( $CO_2$ ) produced. The gaseous mixture after combustion occupied $70 cm^3$ . This mixture consists of $CO_2$ and unreacted $O_2$ . When this mixture was passed through

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Quick Answer

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

Asked on April 28, 2026Chemistry

This chemistry question involves key chemical concepts and calculations. The detailed solution below walks through each step, from identifying the reaction type to computing the final answer.

ScanSolve AI AnswerAnswered on April 28, 2026

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))O_2(g) → xCO_2(g) + (y)/(2)H_2O(l) Step 2: Determine the volume of carbon dioxide (CO_2) produced. The gaseous mixture after combustion occupied 70 cm^3. This mixture consists of CO_2 and unreacted O_2. When this mixture was passed through