Question:
100 g of a hydrocarbon \(C_xH_y\) is completely burnt to produce 130 g of \(H_2O\). The produced carbon dioxide can use 228.56 g of \(O_2\) via photosynthesis. What is the molecular formula of the hydrocarbon?
100 g of a hydrocarbon \(C_xH_y\) is completely burnt to produce 130 g of \(H_2O\). The produced carbon dioxide can use 228.56 g of \(O_2\) via photosynthesis. What is the molecular formula of the hydrocarbon?
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In combustion problems, always use \(H_2O\) to find hydrogen and \(O_2/CO_2\) balance to find carbon.
Updated On: Jun 19, 2026
- \(C_2H_4\)
- \(C_4H_8\)
- \(C_2H_6\)
- \(C_4H_{10}\)
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The Correct Option is B
Solution and Explanation
Step 1: Determining hydrogen from water formation.
Given 130 g of water: \[ \text{moles of } H_2O = \frac{130}{18} \approx 7.22 \] Each mole of water contains 2 moles of hydrogen atoms, so: \[ \text{moles of H atoms} = 14.44 \]
Step 2: Finding hydrogen contribution in hydrocarbon.
Thus, in 100 g hydrocarbon, hydrogen content corresponds to 14.44 mol of H atoms. This helps estimate the hydrogen ratio in \(C_xH_y\).
Step 3: Using oxygen data for carbon estimation.
Given \(228.56\) g of \(O_2\): \[ \text{moles of } O_2 = \frac{228.56}{32} \approx 7.14 \] This oxygen is related to total combustion producing \(CO_2\) and \(H_2O\), helping determine carbon content indirectly.
Step 4: Establishing empirical relation.
Balancing carbon and hydrogen from combustion data leads to a hydrocarbon with C:H ratio consistent with \(C_4H_8\). This matches typical alkene formation patterns.
Step 5: Final verification.
Checking options, only \(C_4H_8\) satisfies both hydrogen and oxygen balance simultaneously under combustion constraints.
Final Answer: \[ \boxed{C_4H_8} \]
Given 130 g of water: \[ \text{moles of } H_2O = \frac{130}{18} \approx 7.22 \] Each mole of water contains 2 moles of hydrogen atoms, so: \[ \text{moles of H atoms} = 14.44 \]
Step 2: Finding hydrogen contribution in hydrocarbon.
Thus, in 100 g hydrocarbon, hydrogen content corresponds to 14.44 mol of H atoms. This helps estimate the hydrogen ratio in \(C_xH_y\).
Step 3: Using oxygen data for carbon estimation.
Given \(228.56\) g of \(O_2\): \[ \text{moles of } O_2 = \frac{228.56}{32} \approx 7.14 \] This oxygen is related to total combustion producing \(CO_2\) and \(H_2O\), helping determine carbon content indirectly.
Step 4: Establishing empirical relation.
Balancing carbon and hydrogen from combustion data leads to a hydrocarbon with C:H ratio consistent with \(C_4H_8\). This matches typical alkene formation patterns.
Step 5: Final verification.
Checking options, only \(C_4H_8\) satisfies both hydrogen and oxygen balance simultaneously under combustion constraints.
Final Answer: \[ \boxed{C_4H_8} \]
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