I find calculations much easier than rote learning stuffwhy are these questions so easy
sorry but like yeah. NO shipwrecks is easier than industrial by far. No calculations, nothing. All rote and stuff.
Since no one is answering,
btw how many marks?
)
PRODUCTION OF OCTYL ETHANOATEIndustrial dominated m8.
Industrial > Shipwrecks.
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I actually got my own timetable wrong, 3U isn't until Nov 5. It's 2U on the same day as EE1. And EE1 might not have to count, but come on, it's harder. But then again, Latin extension sounds harder than French, so we're probably about equal in misfortune.
- Did not explain importance of reflux, keeps volatile products and reactants in the flask.produce ester: let's make ethyl butanoate
1) Add 30 ml Ethanol and 20 ml butanoic acid to a round bottomed flask. Excess of the ethanol is added coz it's cheaper #cheapos
2) Add 5ml of concentrated sulphuric acid (as a dehydrating agent to shift the equilibrium in the forward direction --> increas yield of ester AND it's a catalyst so it increases the rate of the reaction making it go faster) and add some ceramic boiling chips (anti bumping granules to allow the even heating of the liquid and to increase surface area for vaporisation to occur on)
3) Attach a condenser to the the round bottomed flask with the reactants and stuff in it (used because the system is in equilibrium and if the reactants evaporate then like the equilibrium will shift in the reverse direction and reduce yield of ester which is bad). The round bottomed flask is placed in a water bath to allow even heating of water BUT a better thing to use is the heat plate because the reactants are volatile. I think in hsc we should write that we used a heat plate lol. cheap schools.
4) Anyway next put the Bunsen Burner on top of a heat mat and put it under the reaction vessel. (or use the heat plate)
5) Pass the cooling water through the condenser so it condenses the reactants, preventing evaporation and preventing the equilibrium from shifting to the left. Turn on Bunsen burner and the reaction occurs for half an hour at 100 degrees Celsius.
6) then after 30 mins, turn off the Bunsen burner and let the cooling water pass through for a while. after it's cooled, take the round bottomed flask and pour the ester mixture into a separating funnel. 20 ml of NAHCO3 was added to the separaring funnel, this is because NaHCO3 is amphiprotic and it acts as a base :. neutralising the excess butanoic acid which may remain unused in the reaction. The mixture was shaken and left to stand. The lower aqueous layer was drained off.
7) then add 20ml of DISTILLED WATER to the separating funnel. Since water is a polar substance, it would dissolve the excess polar ethanol if there is any because likes dissolve likes. Again shake it and drain off the lower aqueous layer leaving only the ester and you've successfully purified the ester ethyl butanoate (I hope
Pretend I drew the diagram and the equilibrium equation for refluxing
k done
now mark it
woops
The question
bs how can you give me 2/7 for that?
I never did this part and I didn't even realise we were supposed to. You say that you use an amphiprotic solution to act as a base, is the reason you do this instead of just using a base so you can add it in excess without disrupting the pH excessively?produce ester: let's make ethyl butanoate
1) Add 30 ml Ethanol and 20 ml butanoic acid to a round bottomed flask. Excess of the ethanol is added coz it's cheaper #cheapos
2) Add 5ml of concentrated sulphuric acid (as a dehydrating agent to shift the equilibrium in the forward direction --> increas yield of ester AND it's a catalyst so it increases the rate of the reaction making it go faster) and add some ceramic boiling chips (anti bumping granules to allow the even heating of the liquid and to increase surface area for vaporisation to occur on)
3) Attach a condenser to the the round bottomed flask with the reactants and stuff in it (used because the system is in equilibrium and if the reactants evaporate then like the equilibrium will shift in the reverse direction and reduce yield of ester which is bad). The round bottomed flask is placed in a water bath to allow even heating of water BUT a better thing to use is the heat plate because the reactants are volatile. I think in hsc we should write that we used a heat plate lol. cheap schools.
4) Anyway next put the Bunsen Burner on top of a heat mat and put it under the reaction vessel. (or use the heat plate)
5) Pass the cooling water through the condenser so it condenses the reactants, preventing evaporation and preventing the equilibrium from shifting to the left. Turn on Bunsen burner and the reaction occurs for half an hour at 100 degrees Celsius.
6) then after 30 mins, turn off the Bunsen burner and let the cooling water pass through for a while. after it's cooled, take the round bottomed flask and pour the ester mixture into a separating funnel. 20 ml of NAHCO3 was added to the separaring funnel, this is because NaHCO3 is amphiprotic and it acts as a base :. neutralising the excess butanoic acid which may remain unused in the reaction. The mixture was shaken and left to stand. The lower aqueous layer was drained off.
7) then add 20ml of DISTILLED WATER to the separating funnel. Since water is a polar substance, it would dissolve the excess polar ethanol if there is any because likes dissolve likes. Again shake it and drain off the lower aqueous layer leaving only the ester and you've successfully purified the ester ethyl butanoate (I hope
Pretend I drew the diagram and the equilibrium equation for refluxing
k done
now mark it
I gave the question 2/7! I'd personally give your answer 7 if it had the reaction equation.
Oh sorry sorry! Yeah it was not great with wording
It's cool, how could I give your answer 2 when mine was worse? haha
.Industrial dominated m8.
Industrial > Shipwrecks.
For 7 marks, that's what they're looking for. Chemistry is like that, they go way out of the question and require you to write additional info.
Potentially yes. I never paid much attention to why it is used but yeah I'm assuming it's also because it produces CO2 (fizzing) since acid + carbonate gives you salt + CO2 + water, and by using NaHCO3 as amphiprotic/amphoteric substance, the heat released in the exothermic neutralisation reaction is much less than if a strong base were used so it is safer in a sense, I suppose.
ahaha all good.
What did you get?
What did you get?
*facepalm*
haha do the question, it's a multiple choice.