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CH3CH2CH2OH + 4.5O2------>3CO2 + 4H2O1) In an experiment 12.0dm3 of oxygen measured under room conditions is used to burn completely 0.10mol of propan-1-ol. What is the final volume of gas measured at room conditions? ANS: 8.40dm3
Anyone can explain?
Take a piece of paper, jot down all formulas, conversions and neseccary things. Group them up orderly. REvise it again and againcan anyone give me some tips to excel in AS and A2 Organic Chemistry..............pleaseeeeee
and stick on the door of toiletTake a piece of paper, jot down all formulas, conversions and neseccary things. Group them up orderly. REvise it again and again
Forgot to mention xDand stick on the door of toilet
CH3CH2CH2OH + 4.5O2------>3CO2 + 4H2O
so 0.1 mol propanol reacts with 0.45 mol of the o.5 mol oxygen provided (12dm3 oxygen is 0.5 mol)
0.05 mol of oxygen is left over as gas.
0.3 mol of CO2 is formed which is the gaseous product as H2O will be liquid at r.t.p.
0.35mol of total gases.
0.35x24=8.4dm3 gases in the final mixture under ROOM CONDITIONS.
Can someone please solve this question and solve it? c part ii nov 2016 paper 52
View attachment 61984
View attachment 61985
2-x : x/2 : x
In essence, it's a pretty simple question if you ask me. People tend to get confused seeing variables instead of constants.
Anyhow.
There are two approaches to this.
One is quicker but much more confusing. If you want, let me know and I'll enlist that too.
If not, simply take the equations and manipulate.
A- Inital: 2 : 0 : 0
Final : 2-x: 2x : x
Total moles: 2-2+2x+x = 3x so A is incorrect.
B-
Initial: 2 : 0 : 0
Final: 2-2x : 2x : x
Total moles: 2-2x+2x+x = 2+x so B is incorrect
C-
Initial: 2 : 0 : 0
Final 2-2x:x:x
Total = 2-2x+x+x = 2
D-
Initial: 2 : 0 : 0
Final: 2-x : x/2 : x [x = 2R]
Total moles = 2-x+x/2+x =2+x/2 mols!
help pleaseeeeee!View attachment 62015
pls explain all briefly. Starting from part (ii)
remember Ag2SO4 partially soluble.
paper is m/j 2015 p43
Thanks!!
Could someone please help me with a problem on May/June 2014/P23...question #2
I am having difficulty understand (iv). It says, "Calculate the amount, in moles, of ammonium ions in the sample of the double salt'. From what I see on the marking scheme, it is saying the NH4+ react with the H+ in a 1:1 ration. I dont understand where this 1:1 ration is coming from? The only equation that is written is
NH4+ + OH- -----> NH3 + H2O
thanks
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