Question:
What are \(x\) and \(y\) in the following reaction?
\[
x\mathrm{Pb_3O_4}\rightarrow y\mathrm{PbO}+O_2
\]
What are \(x\) and \(y\) in the following reaction?
\[ x\mathrm{Pb_3O_4}\rightarrow y\mathrm{PbO}+O_2 \]
\[ x\mathrm{Pb_3O_4}\rightarrow y\mathrm{PbO}+O_2 \]
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Always balance metal atoms first and then balance oxygen or hydrogen atoms at the end.
Updated On: Jun 15, 2026
- \(x=3,\ y=6\)
- \(x=2,\ y=4\)
- \(x=2,\ y=5\)
- \(x=2,\ y=6\)
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The Correct Option is D
Solution and Explanation
Step 1: Write the given reaction.
\[ x\mathrm{Pb_3O_4}\rightarrow y\mathrm{PbO}+O_2 \]
We need to balance the equation to determine the values of \(x\) and \(y\).
Step 2: Balance lead atoms.
Each molecule of \(\mathrm{Pb_3O_4}\) contains \(3\) lead atoms.
Taking \(2\mathrm{Pb_3O_4}\), total lead atoms become
\[ 2\times3=6 \]
Therefore, on the product side we must have
\[ 6\mathrm{PbO} \]
Thus,
\[ x=2,\quad y=6 \]
Step 3: Verify oxygen atoms.
On the left side, oxygen atoms are
\[ 2\times4=8 \]
On the right side, oxygen atoms are
\[ 6\text{ from }6\mathrm{PbO}+2\text{ from }O_2 \] \[ =8 \]
Hence, the equation is balanced.
Step 4: Write the balanced equation.
\[ 2\mathrm{Pb_3O_4}\rightarrow6\mathrm{PbO}+O_2 \]
Step 5: Final conclusion.
Therefore,
\[ \boxed{x=2,\ y=6} \]
\[ x\mathrm{Pb_3O_4}\rightarrow y\mathrm{PbO}+O_2 \]
We need to balance the equation to determine the values of \(x\) and \(y\).
Step 2: Balance lead atoms.
Each molecule of \(\mathrm{Pb_3O_4}\) contains \(3\) lead atoms.
Taking \(2\mathrm{Pb_3O_4}\), total lead atoms become
\[ 2\times3=6 \]
Therefore, on the product side we must have
\[ 6\mathrm{PbO} \]
Thus,
\[ x=2,\quad y=6 \]
Step 3: Verify oxygen atoms.
On the left side, oxygen atoms are
\[ 2\times4=8 \]
On the right side, oxygen atoms are
\[ 6\text{ from }6\mathrm{PbO}+2\text{ from }O_2 \] \[ =8 \]
Hence, the equation is balanced.
Step 4: Write the balanced equation.
\[ 2\mathrm{Pb_3O_4}\rightarrow6\mathrm{PbO}+O_2 \]
Step 5: Final conclusion.
Therefore,
\[ \boxed{x=2,\ y=6} \]
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