4 NH3 +5 02 +4NO + 6H2O When 70.25 grams of NH3 react, how many moles of H20 are produced?
1 answer:
Answer:
6.19 mol H₂O
Explanation:
- 4 NH₃ + 5O₂ → 4NO + 6H₂O
First, we<u> convert 70.25 grams of NH₃ into moles</u>, using its<em> molar mass</em>:
- 70.25 g ÷ 17 g/mol = 4.13 mol NH₃
Then we <u>convert 4.13 moles of NH₃ into moles of H₂O</u>, using the <em>stoichiometric coefficients of the balanced reaction</em>:
- 4.13 mol NH₃ *
= 6.19 mol H₂O
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Moles of solute for both a and b are the same = 1 mol
<h3>Further explanation</h3>Given
a 500 cm³ of solution, of concentration 2 mol/dm³
b 2 litres of solution, of concentration 0.5 mol/dm³
Required
moles of solute
Solution
Molarity shows the number of moles of solute in every 1 liter of solution or mmol in each ml of solution
Can be formulated :
a.
V = 500 cm³ = 0.5 L
M = 2 mol/L
n=moles = M x V
n = 2 mol/L x 0.5 L
n = 1 mol
b.
V = 2 L
M = 0.5 mol/L
n=moles = M x V
n = 0.5 mol/L x 2 L
n = 1 mol