can someone PLEASE help with the above problem..given the reaction below...what
ID: 855839 • Letter: C
Question
can someone PLEASE help with the above problem..given the reaction below...what mass of KO2, in grams, is required to react with CO2 at STP and standard colar volume?
PLEASE explain each step you perform. I have submitted this question 3 different times and haven't gotten an answer i understand yet!!! one answer said it was unfinished, but this is all i was given...another response just solved the problem and didnt explain anything, so i couldnt follow the answer....PLEASE HELP!!!!!
A gaseous chlorofluorocarbon, CClxFy, contains 11 .79% C, 69.57% Cl, and 18.64% F. You find that 0.107 g of the compound fills a 458 mL flask at 25 degree C with a pressure of 21.3 mmHg. What is the empirical formula, molar mass, and molecular formula of the chlorofluorocarbon. Given the reaction below What mass of KO2, in grams, is required to react with CO2 at STP and standard molar volume?Explanation / Answer
given ;
11.79% C ; 69.57% Cl ; 18.64% F
we know PV = nRT
P = 21.3 mmhg = 0.028atm ; V = 0.458 ; T = 25 = 298K
R = 0.0821 ; n= m/M m= mass = 0.107gms ; M = molecular weight
keeping all values ;
M[molar mass of copound] = 204.13gms
mass of C = 11.79 * 204.13/100 = 24.06 gms = 2 carbons atoms[MW of C = 12]
mass of Cl = 69.57*204.13/100 = 142.01gms = 4 chlorine atoms[MW of Cl = 35.45]
mass of F = 38.13 = 2 flourine atoms [MW of F = 19]
Molecular formula = C2Cl4F2 Empirical formula = CCl2F
from the reaction we can say that ;
4 moles of KO2 reacts with 2 moles of CO2
given conditions are STP and Molar volume.
at STP and molar volume conditions we can say that 1 mole of CO2 is available
since 1 Mole of gas at STP occupies 22.4 litres [molar volume]
for 2 moles of CO2 there is 4 moles of KO2 .......
for 1 mole of CO2 there is 2 moles of KO2 =====> 142.18gms
therefore 142.18gms of KO2 is needed to react with CO2 at given conditions.
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