Question

Use stoichiometry calculations and show all work:

calculate how many grams of water one could produce if 3.35 grams of H3PO4 react completely.
Reaction: H3PO4(aq) + 3LiOH(aq) = 3H2O(l) + Li3PO4(aq)

Answer 1

Step-by-step explanation:

To calculate the amount of water produced from the reaction of H3PO4 and LiOH, we can use stoichiometry. We will use the balanced chemical equation:

H3PO4(aq) + 3LiOH(aq) = 3H2O(l) + Li3PO4(aq)

The equation tells us that 1 mole of H3PO4 reacts with 3 moles of LiOH to produce 3 moles of H2O and 1 mole of Li3PO4.

First, we need to convert the amount of H3PO4 (3.35 g) to moles:

3.35 g H3PO4 / 98 g/mol = 0.0342 mol H3PO4

Next, we'll use the mole ratio from the balanced equation to determine the amount of LiOH required:

0.0342 mol H3PO4 * (3 mol LiOH / 1 mol H3PO4) = 0.1026 mol LiOH

Finally, we'll use the mole ratio from the balanced equation to determine the amount of water produced:

0.0342 mol H3PO4 * (3 mol H2O / 1 mol H3PO4) = 0.1026 mol H2O

Converting the amount of water produced (0.1026 mol) to grams:

0.1026 mol H2O * 18 g/mol = 1.84 g H2O

So, if 3.35 grams of H3PO4 react completely with LiOH, 1.84 grams of water would be produced.