Question:
For the reaction represented by the equation,
\[
CX_4 + 2O_2 \rightarrow CO_2 + 2X_2O
\]
9.0 g of CX$_4$ completely reacts with 1.74 g of oxygen. The approximate molar mass of X will be
For the reaction represented by the equation,
\[
CX_4 + 2O_2 \rightarrow CO_2 + 2X_2O
\]
9.0 g of CX$_4$ completely reacts with 1.74 g of oxygen. The approximate molar mass of X will be
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Always follow: mass $\rightarrow$ moles $\rightarrow$ mole ratio $\rightarrow$ unknown.
Updated On: Apr 23, 2026
- 20
- 40
- 60
- 80
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The Correct Option is D
Solution and Explanation
Concept:
Use mole concept and stoichiometric ratio from balanced equation.
Step 1: Calculate moles of O$_2$:
\[ \text{Moles of } O_2 = \frac{1.74}{32} = 0.054375 \]
Step 2: Use stoichiometry (2 mol O$_2$ reacts with 1 mol CX$_4$):
\[ \text{Moles of } CX_4 = \frac{0.054375}{2} = 0.0271875 \]
Step 3: Find molar mass of CX$_4$:
\[ \text{Molar mass} = \frac{9.0}{0.0271875} = 331 \]
Step 4: Calculate atomic mass of X:
\[ 12 + 4X = 331 \] \[ 4X = 319 \Rightarrow X = 80 \] Conclusion:
Atomic mass of X = 80
Step 1: Calculate moles of O$_2$:
\[ \text{Moles of } O_2 = \frac{1.74}{32} = 0.054375 \]
Step 2: Use stoichiometry (2 mol O$_2$ reacts with 1 mol CX$_4$):
\[ \text{Moles of } CX_4 = \frac{0.054375}{2} = 0.0271875 \]
Step 3: Find molar mass of CX$_4$:
\[ \text{Molar mass} = \frac{9.0}{0.0271875} = 331 \]
Step 4: Calculate atomic mass of X:
\[ 12 + 4X = 331 \] \[ 4X = 319 \Rightarrow X = 80 \] Conclusion:
Atomic mass of X = 80
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