One question I need help on!!?

Question

its a volume question:

How many liters of oxygen (O2) are needed to convert 100 liters of hydrogen (H2) to water (H2O)?

Answer 1

Assuming the ideal gas law there are approximately 22.4 L/mole of gas if we assume all of this is occuring at STP. Therefore, from the data given we know that there are 100/22.4 moles of hydrogen.

Creating a reaction expression:

2 H2 + O2 ==> 2H2O

So we know that for every 2 moles of hydrogen, one mole of oxygen is needed. Therefore, we need 100/22.4/2 moles of oxygen. We can once more apply the factor 1 mol/22.4L to get 22.4*100/22.4/2 litres of oxygen.

Simplifying we get 50 litres of oxygen will be needed.

Answer 2

This is the question of multiple choice and you can instantly solve such type of questions in future. The answer for your question is 50 ltrs. How ? I am telling you.
The product formed by combining H2 and O2 is H2O and in H2O the atomicity of H is 2 while that of O is 1 so the combining ratio between the reactants (H & O) is 2:1 therefore the volume of Oxygen needed to convert 100 ltrs. of H2 to water is half (50 %) of the volume of H2 that is 50 ltrs.

Answer 3

I might be wrong but.. 100 moles of H20 will contain 100 moles of H2 and Oxygen. Since you have O2 instead of O, you will need half as much or 50 liters of oxygen. (I know that liters and moles are different, but since the temperature/pressure is not given, I would assume it is constant which makes them drop from the equation when you convert)

Answer 4

50, assuming the pressure and temperature are the same
2H2 +O2= 2H2O

Answer 5

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Answer 6

50?