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

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 $9.0 \mathrm{~mol} \mathrm{H}_{3} \mathrm{PO}_{4}$ ? [?] $\mathrm{mol} \mathrm{Na}_{3} \mathrm{PO}_{4}$
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Solution

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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 \(\mathrm{H}_{3} \mathrm{PO}_{4}\).

\[ \text{Moles of } \mathrm{Na}_{3} \mathrm{PO}_{4} = 9.0 \text{ moles} \]

Final Answer

\[ \boxed{9.0 \text{ moles of } \mathrm{Na}_{3} \mathrm{PO}_{4}} \]

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