if 2.0 moles of magnesium hydroxide are present, how many moles of phosphoric acid, would be required for…

if 2.0 moles of magnesium hydroxide are present, how many moles of phosphoric acid, would be required for the reaction? 3mg(oh)₂ + 2h₃po₄ → mg₃(po₄)₂ + 6h₂o\na 1.33 mol\nb 0.33 mol\nc 3.0 mol\nd none of the above

if 2.0 moles of magnesium hydroxide are present, how many moles of phosphoric acid, would be required for the reaction? 3mg(oh)₂ + 2h₃po₄ → mg₃(po₄)₂ + 6h₂o\na 1.33 mol\nb 0.33 mol\nc 3.0 mol\nd none of the above

Answer

Answer:

A. 1.33 mol

Explanation:

Step1: Identify mole - ratio

From the balanced equation $3Mg(OH)_2 + 2H_3PO_4\rightarrow Mg_3(PO_4)_2+6H_2O$, the mole - ratio of $Mg(OH)_2$ to $H_3PO_4$ is $3:2$.

Step2: Set up proportion

Let $x$ be the moles of $H_3PO_4$. We have the proportion $\frac{3}{2}=\frac{2.0}{x}$.

Step3: Solve for $x$

Cross - multiply: $3x = 2\times2.0$. Then $x=\frac{2\times2.0}{3}=\frac{4.0}{3}\approx1.33$ mol.