how many moles of o2(g) are needed to react completely with 52.0l of ch4(g) at stp to produce co2(g) and h2o(g?
how many moles of o2(g) are needed to react completely with 52.0l of ch4(g) at stp to produce co2(g) and h2o(g) according to the reaction: ch4(g) + 2o2(g) -- co2(g) + 2h2)(g)? Please help
- 7 years agoFavorite Answer
At STP 1 mole of a gas has a volume of 22.4L at 1 atm. So, a volume of 52.0L= x moles of CH4(g) at 1 atm. Use identity and solve for mole of CH4(g):
x moles of CH4(g)/52.0L=1 mole/22.4L
x moles of CH4(g)=(52.0L/22.4L)
2.321 moles of CH4(g) at STP
The reaction shows that 1 mole of CH4=2 moles of O2. Solve for moles of O2:
2.321 moles of CH4*(2 moles of O2/1 mole of CH4)=4.642=4.64 moles of O2
***Answer contains only 3 significant figures.
I like to keep an extra digit while performing calculations and round off at the very end. It usually makes a difference when calculating an answer exactly like what is given in the key.