If 45.6 grams of water decomposes at 301 Kelvin and 1.24 atmospheres, how many liters of oxygen gas can be produced? Show all of the work used to solve this problem.

2 H2O (l) yields 2 H2 (g) + O2 (g)
Hey I just wanted to know if any of you guys can help me figure out this question please and not just the answer it would be great thank you.

Question

If 45.6 grams of water decomposes at 301 Kelvin and 1.24 atmospheres, how many liters of oxygen gas can be produced? Show all of the work used to solve this problem. 

2 H2O (l) yields 2 H2 (g) + O2 (g)
Hey I just wanted to know if any of you guys can help me figure out this question please and not just the answer it would be great thank you.

dtan5457 · Answer

You need the ideal gas law here, which is pV=NRT
p=pressure
v=volume
n=# of moles
t=temperature
r=molar gas content (0.0821)

You get the amount of moles there are for oxygen based on h2o.

2h2o=36 grams

45.6/36=1.27 moles

there are 1.27 moles of oxygen

now just plug everything in

dtan5457 · Answer

remember you are solving for V

dtan5457 · Answer

V = nRT / P = (1.27)(0.0821)(301) / (1.24) = 25.2 L O2

anonymous · Answer

oh so that would be the step by step process to do ths type of question? thanks this really helped a lot!