At STP 4.83 L of chlorine is produced during a chemical reaction. What is the mass of this gas? Answer in unites of g.
(please include all decimal places; no sig figs, float)
2007-11-01 14:25:00 · 3 answers · asked by The Wind 2 in Science & Mathematics ➔ Chemistry
thnx guys....
the UT hwk service thing keeps saying that 15.309375 is wrong....oh well....il just tell the professor
2007-11-01 14:48:05 · update #1
Atomic weight: Cl=35.5 Cl2=71
4.83LCl2 x 1molCl2/22.4LCl2 x 71gCl2/1molCl2 = 15.309375g Cl2
2007-11-01 14:29:55 · answer #1 · answered by steve_geo1 7 · 0⤊ 0⤋
I personally refuse to give you the answer, though i willl tell you how to work it. Firstly you need to figure out how many moles of gas you have. at STP, one mole of a gas is 22.4 liters, so divide 4.83 by 22.4. now you have to calculate the molar mass of chlorine; this one is easy, just look on your periodic table. now divide your number of moles of the chlorine gas by your molar mass, that will give you your answer. (remember that chlorine gas is Cl2 as it needs to bind with something)
2007-11-01 21:32:56 · answer #2 · answered by Michael R 2 · 0⤊ 0⤋
PV=nRT
n=m/M
m=molarmass Cl*1atm*4.83L/(.082*273.15)
2007-11-01 21:31:43 · answer #3 · answered by Crazy and Lovin It 4 · 0⤊ 0⤋