Question

Acetic acid contains carbon,hydogen and oxygen. 4324g of sample acetic acid on complete combustion gave 6.21g of CO_2 and 2.54g of H_2O. The Molecular mass of acetic acid is 60. Find
(i) Empirical formula of acetic acid
(ii) Molecular formula of acetic acid

Answer 1

Can you draw a table for finding empirical formula?

Answer 2

Step 1 = % of elements
Step 2 =Mole Ratio
step 3 = Simplest Ratio
Step 4 = Establishing emp. formula

Answer 3

Although i am good at this........but this question is crazy....cant just get it done

Answer 4

Example Question : 1.8g of an organic compound on combustion gave 3.21g CO2 AND 1.322g H2O. Calculate Empirical Formula.
Step 1 % of elements :
C= 12/44 * 3.21/1.8 * 100 = 48.63%
H=2/18*1.322/1.8 * 100 = 8.16 %
O = 100-(48.63+8.16)=43.21%

Step 2 Mole Ratio :
C= 48.63/12 = 4.05
H= 8.16/1 = 8.16
O= 23.21/16 = 2.7

Step 3 Simplest Ratio :
C=4.05/2.7 = 1.5
H=8.16/2.7 = 3
O=2.7/2.7
In order to get nearest whole no. ratio,all are multiplied by 2
Hence C=3 , H=6 , O=2

Step 4 Establishing Empirical Formula:
C_3H_6_O_2

Answer 5

^here is a example

Answer 6

but the question i've asked is similar to this but it is entirely different ...it is giving crazy simplest ratio

Answer 7

Hold on

Answer 8

okay

Answer 9

4324g of sample acetic......
is the number correct?????

Answer 10

yes it is

Answer 11

1,69 gr C
0.28 gr H
4324-1,69-0.28=4322.03 gr of oxyxen !!!!!
something is wrong!!!

Answer 12

it is from a question paper....and it is correct

Answer 13

is CO2 and H2O in gr or in Kgr ????

Answer 14

it is the 1st question i've asked

Answer 15

i see it.
i still thing the numbers are wrong.
try to take CO2 and H2O in Krg to see if it make sense....

Answer 16

4.324 kg acetic acid will produce only 6.21 g of CO2 and 2.54 H2O . Not possible, I think.

Answer 17

okay....this is what i think
since you know the compound is acetic acid, then you should know it has a molecular formula C2H4O2 and an empirical formula of CH2O.....