- #1
jegues
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Homework Statement
Ethylene oxide is produced industrially from the reaction of ethylene with oxygen at atmospheric pressure and 283 oC, in the presence of silver catalyst.
[tex]C_{2}H_{4} + O_{2} \rightarrow C_{2}H_{4}O[/tex]
Assuming 100 % yield, how many kg of ethylene oxide can be produced from 35100 L of a mixture containing ethylene and oxygen in 1:1 molar ratio?
Homework Equations
The Attempt at a Solution
First I balanced the equation like so,
[tex]2C_{2}H_{4} + O_{2} \rightarrow 2C_{2}H_{4}O[/tex]
I then converted the temp. from celsius to kelvin so,
525.15K
I'm not sure what value I should use for pressure, in a question like this am I just assuming that P = 1atm?
I then applied PV= nRT and solved for moles. Once I have the number of moles I used the molar mass to get it into grams and then I converted grams to kilograms.
I still got the answer wrong however.
What am I doing wrong?
EDIT:Also, what value for the gas constant do I use that will work with the units K, mol, atm, and L?
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