Question

Can some one help me with gas calculations??

Answer 1

sure!!

Answer 2

omg thank you! I do not understand this at all!

Answer 3

If 3.0 liters of oxygen gas react with excess carbon monoxide at STP, how many liters of carbon dioxide can be produced under the same conditions?

2 CO (g) + O2 (g) yields 2 CO2 (g)

Answer 4

that is easy!!
you have to look at the equation and see how many mol of O2 and moles of CO2 you have

one mol of ANY gas at STP condition has the same volume.
so if you have 1mol of O2 that produce 1mol of CO2 you will have the same volume of CO2 produced than the O2 consumed in the reaction.

now if in the reaction you have 1mol O2 that produce 5 mol of CO2 then the volume of the CO2 is going to be 5 times more than the volume of the O2 consumed in the reaction

Answer 5

im still a little confused..

Answer 6

tell me how many mol of O2 you see in the equation?

Answer 7

I see 2

Answer 8

NO!
O2 the 2 is the sub-index that indicate how many atoms per molecule you have to look at the prefix, if there is no number before the O2 means that is 1.
2 O2 = 2 mol O2

Answer 9

now how many mol of O2 do you see in the equation and how many mol of CO2 do you see in the equation

Answer 10

1 O2 and 2 CO2

Answer 11

PERFECT!!!

Answer 12

okay good!

Answer 13

Now the amount of moles from O2 to CO2 increase by 2 then the volume will increase also by 2

Answer 14

so 6?

Answer 15

3.0 L O2 x 2 mol CO2/ 1 mol O2 = 6 L CO2

Answer 16

do you have more?

Answer 17

Thank you so much!!

Answer 18

and yes

Answer 19

How many liters of methane gas (CH4) need to be combusted to produce 8.5 liters of water vapor, if all measurements are taken at the same temperature and pressure? Show all of the work used to solve this problem.

CH4 (g) + 2 O2 (g) yields CO2 (g) + 2 H2O (g)

Answer 20

what do you think? how many mol of CH4 you have in the equation and how many moles of H2O you have in the equation?