Question

Can somebody help me with three Gas Stoichemistry questions? The first one is:
How many liters of water can be made from 55 grams of oxygen gas and an excess of hydrogen at STP?

Answer 1

Since H2 is in excess, the amount of water will depend on the amount of O2. Can you write out the balanced chemical equation?

Answer 2

The chemical equation would be 2H2 + O2 -> 2H2O

Answer 3

And sorry for the late response >_<

Answer 4

Right. So you can see that the ratio of O2 to H2O is 1:2. Therefore, the amount of H2O produced will be the same as twice the amount of O2 you have,

Answer 5

Okay so Oxygen is 55 grams, so Water is 110 grams. And 1 gram of H2O is equal to 0.001 liters, so 110 grams of water would equal to 0.11 liters? Is that the answer?

Answer 6

Well no you have to use their number of moles for that and not just the mass.

Answer 7

The number of moles in Oxygen is 1.72, right?

Answer 8

Yup.

Answer 9

So the number of moles in H20 is 3.44? Then what do I do?

Answer 10

Yes. And then you will find the mass of water again. And then you use the density of water to find the volume.

Answer 11

I got 77 L of H2O, is that right?

Answer 12

Let's see. So there are 3.44 moles of water. Multiplied by 18 you get 61.92 g. Density of water is 1000g/l. So 1000/61.92