Questions: Unit Exam - Stoichiometry
6.0 mol NaOH reacts with 9.0 mol H3PO4 according to the equation below:
3 NaOH + H3PO4 -> 3 H2O + Na3PO4
How many moles of Na3PO4 could form from 9.0 mol H3PO4?
[?] mol Na3PO4
Transcript text: Unit Exam - Stoichiometry
6.0 mol NaOH reacts with $9.0 \mathrm{~mol} \mathrm{H}_{3} \mathrm{PO}_{4}$ according to the equation below:
\[
3 \mathrm{NaOH}+\mathrm{H}_{3} \mathrm{PO}_{4} \rightarrow 3 \mathrm{H}_{2} \mathrm{O}+\mathrm{Na}_{3} \mathrm{PO}_{4}
\]
How many moles of $\mathrm{Na}_{3} \mathrm{PO}_{4}$ could form from $9.0 \mathrm{~mol} \mathrm{H}_{3} \mathrm{PO}_{4}$ ?
[?] $\mathrm{mol} \mathrm{Na}_{3} \mathrm{PO}_{4}$
Solution
Solution Steps
Step 1: Write the Balanced Chemical Equation
The balanced chemical equation for the reaction is:
\[
3 \mathrm{NaOH} + \mathrm{H}_{3} \mathrm{PO}_{4} \rightarrow 3 \mathrm{H}_{2} \mathrm{O} + \mathrm{Na}_{3} \mathrm{PO}_{4}
\]
Step 2: Identify the Mole Ratio
From the balanced equation, the mole ratio of \(\mathrm{H}_{3} \mathrm{PO}_{4}\) to \(\mathrm{Na}_{3} \mathrm{PO}_{4}\) is 1:1.
Step 3: Calculate the Moles of \(\mathrm{Na}_{3} \mathrm{PO}_{4}\) Formed
Given that we have 9.0 moles of \(\mathrm{H}_{3} \mathrm{PO}_{4}\), and using the 1:1 mole ratio, the moles of \(\mathrm{Na}_{3} \mathrm{PO}_{4}\) formed will be the same as the moles of \(\mathrm{H}_{3} \mathrm{PO}_{4}\).