How do you solve this: if 24.0 L of O2 burns completely a sample of carbon disulfide, how many grams of sulfur dioxide will be produced at 15 degrees celcius at a pressure of 1.3 atm? (the answer is 45.7 g).

Question

CS2 + 3CO2 -> CO2 + 2SO2

Answer 1

I am assuming you meant 24.0L of CO2 not O2.

Use the following formula:

PV=nRT

Where

P=1.3 atm
V=24.0L
n=?
R=0.08205746
T=273.15 + 15=288.15 K

Solve for moles of O2

moles of CO2=n=PV/RT

******1 moles of CO2=2 moles of SO2

moles of CO2*(2 moles of SO2/1 mole of CO2)= moles of SO2

moles of SO2*(64.066 g/mol)= mass of SO2

Answer 2

I made a typo,

it should say

******3 moles of CO2=2 moles of SO2

moles of CO2*(2 moles of SO2/3 mole of CO2)= moles of SO2

moles of SO2*(64.066 g/mol)= mass of SO2

But when I punch in the numbers I am not getting 45.7g but I am getting about 56 g. So, I am not sure about this problem.

Answer 3

the equation is supposed to say:

CS2 + 3O2 -> CO2 + 2SO2

* O2 not 3CO2

Answer 4

Still doesn't change my overall answer.