Question

2 H2(g) + O2(g) → 2 H2O(l) How many moles of H2O are formed from 2.9L of O2 at a temperature of 325K and a pressure of 0.988atm?

Answer 1

PLEASE HELP!!! @iPwnBunnies

Answer 2

You'll need to find how many moles of O2 are there using the Ideal Gas Equation.
\[PV = nRT\]
Where 'n' is the amount of moles of O2. R will be 0.08206 L-atm/mol-K

Answer 3

Then, use simple stiochiometry mole ratio stuff to get the amount of H2O.

Answer 4

So 2.9(.998)=n(0.08206)(325)?

Answer 5

@iPwnBunnies

Answer 6

Yes ma'am.

Answer 7

Ok... can you double check it once I do the math?

Answer 8

Ok.

Answer 9

2.8942=n26.6695

Answer 10

Now what do I do?

Answer 11

Solve for n?

Answer 12

do I subtract the 26.6695 from both sides?

Answer 13

Nooo, divide both sides. It's being multiplied by the 'n'. To undo multiplication, we gotta divide.

Answer 14

.1085=n?

Answer 15

Yep. That's how many moles of O2 we have. Now we use mole ratios to get how much H2O we can make from the O2.
looking at the balanced equation, we can make 2 moles of H2O for every mole of O2.

Answer 16

So my answer is 2 moles for every mole of o2

Answer 17

No. We have to use that ratio to calculate how much H2O we get from 0.1085 moles of O2.

Answer 18

How do I do that?

Answer 19

\[(0.1085 mol O2)*\frac{2 mol H2O}{1 mol O2} = \]

Answer 20

so 2(.1085)

Answer 21

Yep.

Answer 22

so 0.217 mol h20

Answer 23

Yep.

Answer 24

Thank you.. I have one more question if you can help

Answer 25

Just kidding I have 2 more.

Answer 26

Uhhh, idk. I gotta work on stuff myself, sorry. :/

Answer 27

Dang ok thanks,