from the reaction equation ... each mole of H2O results in two moles of HNO3
(moles H2O) * 2 = (moles HNO3) ... ? * 2 = 4.5
How Many Moles Of H2O Are Required To Produce 4.5 Moles Of HNO3 According To The Following Reaction: 3NO2+H2O = 2HNO3+NO
15 answers
student
9mol
2.5
X=2.25 mol
First balance the equation then change the given mole to mass then assume you are asked as a gram then divide the answer to the molar mass of the asked compound without the cofficent then the answer is 2.25
x/4.5=126/2
X=28.35
X=28.35
Student
Teacher
2.25
3no2+h2o_2hno3+no
2.25
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 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.
2.25
The answer is 2.25 moles of H2O.