how many grams of silicon tetrafluoride, a gas, at room temperature, would fill the same volume as that occupied by 295 grams of carbon monoxide at 75 degrees C and 575 torr?
2006-12-27 08:41:57 · 2 answers · asked by rishelly2528 1 in Science & Mathematics ➔ Chemistry
change 295 grams of CO to moles of CO by dividing by the molecular mass of CO (12 + 16).
You need the same number of moles of SiF4. Now take that number of moles and multiply by the molecular mass of SiF4
(28 + 4 x 19) and you will have grams.
I get 1095 g SiF4
2006-12-27 08:50:17 · answer #1 · answered by The Old Professor 5 · 0⤊ 0⤋
All gases should behave the same. first find the volume that the CO occupies, remember to convert to moles and temperature in Kelvin. Then simply plug the volume of the first equation into the second equation and solve for moles then convert to grams.
Starting equation PV=nRT
equation 1
V1=nRT/P you can determine moles(n). R is the gas constant, T is temp in Kelvin. P is pressure. Make sure that the gas constant you uses torr or you may have to convert torr to atm.
equation 2
PV1/RT=n Remember to change the temp to room temp in Kelvin.
This should work out for you
2006-12-27 16:52:46 · answer #2 · answered by bunja2 3 · 0⤊ 0⤋