For H2(g) + O2(g) → H2O(g) How many moles of O2 is needed to produce 1.2 mole of H2O(g) in a complete reaction?


For H2(g) + O2(g) → H2O(g)

How many moles of O2 is needed to produce 1.2 mole of H2O(g) in a complete reaction?

0.3
0.6
1.2
2.4
none of the above

26.

How many moles of oxygen are formed when 58.6 g of KNO3 decomposes according to the following reaction? ( µKNO3 =101.11 g/mol)

4 KNO3(s) → 2 K2O(s) + 2 N2(g) + 5 O2(g)

0.290
0.580
18.5
0.724
1.73

27.

Ammonia reacts with diatomic oxygen to form nitric oxide and water vapor:

4NH3 + 5O2 → 4NO + 6H2O

When 40.0 g NH3 and 50.0 g O2 are allowed to react, which is the limiting reagent?

( µNH3 =17.03 g/mol; µO2 =32.00 g/mol)

NH3
O2
NO
H2O
No reagent is limiting

28.

For N2(g) + 3H2(g) → 2NH3(g)

From experiment, reacting of 2.80 g N2(g) with excess H2(g) yields 3.10 g NH3(g), determine the percent yield of NH3(g).

( µNH3 =17.00 g/mol; µN2 =28.0 g/mol)

70.0%
30.0%
50.0%
80.0%
60.0%

Step 1 of 2

Given data: H2(g)+O2(g)⟶H2O(g)

 

Find: Determine the number of moles of O2 is needed to produce 1.2 mole of H2O(g).

Explanation:

Number of Moles = Mass of substance / Mass of one mole

 

Step 2 of 2

The balanced chemical equation for the reaction H2​(g)+O2​(g)⟶H2​O(g)

shows a 2:1 mole ratio between H2​ and O2​.

 

This means that for every 2 moles of H2​ consumed, 1 mole of O2​ is needed.

 

If 1.2 moles of H2​O are produced, we can use the ratio to find the corresponding moles of O2​:

Moles of O2 ​= 1.22 moles of H2​O​

Moles of O2 ​= 0.6 moles

Explanation:

Therefore, the correct answer is 0.6.

 

Final solution

Therefore, 0.6 moles of O2 is needed to produce 1.2 mole of H2O(g) in a complete reaction.

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