Chemical Forums
Chemistry Forums for Students => Undergraduate General Chemistry Forum => Topic started by: jylxox on October 23, 2009, 08:55:07 PM
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Calculate the density, g/cm3, of carbon dioxide at 98.0 oC and 807 torr.
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First you need the formula to find density, which is d = PM / RT.
Convert 807 torrs to atm by dividing by 760 torr. 807 torr x (1 atm / 760 torr) = 1.06 atm
Then find the molar mass of carbon dioxide, which is ~44g.
R is a constant. (~0.0821)
Convert 98.0 degree C to K, with is 98 + 273.15 K.
The plug everything in and you are good to do. Also remember that mL=cm3.
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That's what I did.
P= 1.06 atm
M = 44 g
R = .0821
T= 371
(1.06 times 44)/(.0821 times 371) = 1.53
And the system says that the answer is wrong.
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What units is your answer in?
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The units are supposed to be g/cm cubed.
The units are not included in the answer.
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I am not asking what they are supposed to be, but what they ARE. You have calculated density to be 1.53 - of what? Pounds per kilogalon? Stones per cubic meter? Ounces per pint?
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P= 1.06 atm
M = 44 g./mol
R = .0821
T= 371 K
(1.06atm times 44g/mol)/(.0821 times 371K) = 1.53g/cm cubed.
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No. Check your units, especially for R.
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the R is equal to 0.08206, but it still the similar answer.
i dont understand this problem too! someone plz help?!
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I am not asking about numerical value, I am asking about UNITS.
For example - molar mass has units [gram/mole]. What units is ideal gas constant in, when its value is 0.0821?
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He is asking for your units "1.53 what?"
HINT....
If you used an R value = 0.082, the your volume units should be in liters.