When 2.50 mol of Mg3N2 are allowed to react according to the following equation, how many moles of H2O also react?
Mg3N2 + 6H2O ---> 3Mg(OH)2 + 2NH3
15 mol H20
2.5 mol Mg3N2 x (6 mols H2O/1 mol Mg3N2) = mols H2O. Note that the numbers in the factor (that part inside the parentheses) actually are the coefficients in the balanced equation AND that the unit we don't want to keep (mols Mg3N2) cancel and the unit we want at the end (mols H2O) remain unaffected and is the unit for the answer.
15 mols
Well, let's do some math. According to the balanced equation, 1 mole of Mg3N2 reacts with 6 moles of H2O. So if we have 2.50 moles of Mg3N2, we can multiply that by the ratio:
2.50 moles Mg3N2 × (6 moles H2O / 1 mole Mg3N2) = 15.00 moles H2O
So, if 2.50 moles of Mg3N2 react, 15.00 moles of H2O will also react. It's a magical water party!
To find out how many moles of H2O react, we can use the mole ratio provided by the balanced chemical equation. The coefficient in front of H2O is 6, indicating that 6 moles of H2O react with 1 mole of Mg3N2.
Given that 2.50 moles of Mg3N2 are reacting, we can calculate how many moles of H2O will react using the mole ratio:
Moles of H2O = Moles of Mg3N2 × (Moles of H2O / Moles of Mg3N2)
Moles of H2O = 2.50 mol × (6 mol H2O / 1 mol Mg3N2)
Moles of H2O = 2.50 mol × 6
Moles of H2O = 15 mol
Therefore, when 2.50 mol of Mg3N2 are allowed to react, 15 moles of H2O will also react.