I put down as my half equation: 2H+ + 2e- --> H2(s)ok, now.... can someone tell me how hydrogen gets reduced
I put down as my half equation: 2H+ + 2e- --> H2(s)ok, now.... can someone tell me how hydrogen gets reduced
You're right.HUH? Really? But wasn't it what element underwent beta decay to get thorium? so if thorium was the final product then shouldn't the original element be one less since, as you say, beta decay does go up? I'm confuzzled
so does that mean what I put down for the cathode half equation is correct?http://www.boardofstudies.nsw.edu.au/hsc_exams/hsc2008exams/pdf_doc/2008HSC-chemistry.pdf
Q25 , was basically the same as the cell from the CSSA paper, instead of CL gas they used hydrogen for our trial, BOS says the cathode is platinum and that the equation they use for the CL half equation is the same as the one on the data sheet, which is what I did for the trial.
I put down as my half equation: 2H+ + 2e- --> H2(s)
According to the table of standard reduction potentials (given in the CSSA exam) you should have put:so does that mean what I put down for the cathode half equation is correct?
You are right. Thorium was the product. the question was to find which element underwent beta decay to get thoriumHUH? Really? But wasn't it what element underwent beta decay to get thorium? so if thorium was the final product then shouldn't the original element be one less since, as you say, beta decay does go up? I'm confuzzled
at least you didnt miss an entire question....industrial chem last q. just didnt see it
For the half equation at the anode, I put: Ni(s) --> Ni2+ + 2e- (I think that was the anode, can't remember the question exactly)According to the table of standard reduction potentials (given in the CSSA exam) you should have put:
H+ + e- --> 1/2 H2
100% agree with this!sec 1 answers were both weird and easy, MC was screwed..
I thought that too. But I'm not sure exactly how you would put the answer. What you wrote could be right.For the half equation at the anode, I put: Ni(s) --> Ni2+ + 2e- (I think that was the anode, can't remember the question exactly)
I was thinking about putting down what it said on the standard reduction potentials, but then I thought it wouldn't be balanced (since two electrons are being transferred, two must be accepted at the hydrogen end?)
hahah oh man hope so otherwise that's 0 marks for a relatively simple question :/pretty sure it was describe i think, not sure, but i did provide with pros and cons for some reason ..... shouldnt have wasted time :-(
and for the electrolytic cell, i am 95% sure it was just hydrogen getting reduced. that was the one of the two tricky questions in the whole exam.
For the ozone monitoring methods: I think you should have put how it actually worked.hahah oh man hope so otherwise that's 0 marks for a relatively simple question :/
Also for the ozone monitoring methods did anyone actually describe how the methods worked or just gave examples, gave units its measured in (say DU for TOMS) and kept it brief. 1 marker lolol
the hydrogen getting reduced business, what did everyone put as the two reasons as to why it was unsuitable for a commercial cell?
pissweak voltage? source of hydrogen maybe?
I put that down too, and my other reason was that the cell can only produce a voltage at temperatures just above room temperature hahahaa fail. I totally blanked out with that one :mad1:For the hydrogen, I said the voltage, comparing it to a normal dry cell.
My other reason was pretty stupid: "Hydrogen gas is explosive". Lol.
i said this tooo....I said, a eery low voltage and the cost of platinum cathode is to high so its not economically viable.
For a monoprotic acid:for the acid model was it just the same size as it fully dissociated?
for diprotic wouldn't it be double the size for H3O+