given 2CH3OH+3O2->2CO2+4H2O

Question

1. Calculate number of grams of CH3OH required to react with 34.0L of O2 at STP.
2. How many liters of CO2 at 18 degrees Celcius and 6.94 atm are produced when 3.40 mol of CH3Oh is burned completely.
3. What volume of CO2 is produced if 7.11L of O2 at STP reacts with an excess of liquid CH3OH and STP conditions are restored.

Show all work involved.

Answer 1

2CH3OH + 3O2 ==> 2CO2 + 4H2O
1. You know 1 mol O2 at STP will occupy 22.4L. Convert 34.0L O2 to mols. mols = 34.0/22.4 = 1.517 which I would round to 1.52 mols.

Using the coefficients in the balanced equation, convert mols O2 to mols CH3OH. That's 1.52 mols O2 x (2 mols CH3OH/3 mols O2) = 1.01 mols CH3OH.
Now convert mols CH3OH to grams. g = 1.01 x 32 = 32.4 g CH3OH.

The other parts are done the same way. Post your work if you get stuck.

Answer 2

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