Question

PLEASE ANSWER!!!! 30 POINTS!!!!!!!

From previous steps, we know 2.0 mol P4O10 can form 8.0 mol H3PO4 and 8.0 mol H2O can form 5.3 mol H3PO4.

How many moles of H3PO4 can form during the reaction?

mol H3PO4

Answer 1

To determine the number of moles of Ca(OH)2 required to react with 1.36 mol of H3PO4, use the stoichiometry of the balanced equation.

Step-by-step explanation:

To determine the number of moles of Ca(OH)2 required to react with 1.36 mol of H3PO4, we can use the stoichiometry of the balanced equation. According to the equation 3Ca(OH)2 + 2H3PO4 -> Ca3(PO4)2 + 6H2O, we can see that 3 moles of Ca(OH)2 react with 2 moles of H3PO4 to produce 1 mole of Ca3(PO4)2. Therefore, if we have 1.36 mol of H3PO4, we can use the mole ratio to calculate the moles of Ca(OH)2.

(1.36 mol H3PO4) x (3 mol Ca(OH)2 / 2 mol H3PO4) = 2.04 mol Ca(OH)2.

So, 2.04 moles of Ca(OH)2 are required to react with 1.36 mol of H3PO4.