4.8 CYL
Question
How many moles of Ca(OH)2 are required to react with 1.36 mol of H3PO4 to produce Ca3(PO4)2 according to the equation \(3Ca{\left( {OH} \right)_2} + 2{H_3}P{O_4} \to C{a_3}{\left( {P{O_4}} \right)_2} + 6{H_2}O\)?
Step-by-Step Solution
Verified Answer
2.04 mol of Ca(OH)2 are required to react with 1.36 mol of H3PO4 to produce 1.36 mol of Ca3(PO4)2.
1Given data
From the given balanced equation, we can see that 3 moles of Ca(OH)2 reacted with 2 moles of H3PO4.
Therefore, let the number of moles be X.
X moles of Ca(OH)2 react with 1.36 moles of H3PO4.
X= \(\frac{{3 \times 1.36}}{2}\)
X = moles of Ca(OH)2 = 2.04 mol
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