How Many Moles Of H2O Are Required To Produce 4.5 Moles Of HNO3 According To The Following Reaction: 3NO2+H2O = 2HNO3+NO
X=2.25 mol
To solve this problem, we need to use stoichiometry.
From the balanced chemical equation, we can see that 1 mole of H2O is needed to produce 2 moles of HNO3. Therefore, we can set up the following proportion:
1 mole H2O/2 moles HNO3 = x moles H2O/4.5 moles HNO3
where x is the number of moles of H2O needed.
Simplifying the proportion by cross-multiplication, we get:
2x = 4.5
Solving for x, we get:
x = 2.25 moles H2O
Therefore, 2.25 moles of H2O are required to produce 4.5 moles of HNO3.
from the reaction equation ... each mole of H2O results in two moles of HNO3
(moles H2O) * 2 = (moles HNO3) ... ? * 2 = 4.5