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It's year 11, don't worry =P Our maths teacher left us, and we're left behind with a substitute to teach us one of the most challenging topics in the 3 unit course: Binomial probability.

Neither have I. What is it?

Well I wasn't going to try, but now that you've sent a challenge, I shall make an attempt to prove you wrong xD (Although the chances of me failing to do so are quite high, as there is no error, or very insignificant ones) [arsehole mode]The key here, I think, is not so much of the concern of...

o_O line of best fit, perhaps? I'm not sure. Well a 'curve' can actually be used to describe any graph. In maths, people say "The area under the curve of y=x".

All amphiprotic substances are amphoteric, but not necessarily all amphoteric oxides are amphiprotic. I think... I read it off somewhere...Might've been wikipedia, forgot.

No. Only amphiprotic substances.

But if density wasn't given, wouldn't you have to assume 1L = 1 kg? That's what my teacher told me. And I thought molar mass had symbol "M" :confused:

=O Everything you see on the right column of the syllabus.

That is a rule? But it said the molar heat of combustion was -2599 kJ/mol. When you calculate the kJ/g, it doesn't make sense to half it, then do the calculations accordingly. UNLESS The original given value was the heat of combustion per TWO moles because of the 2 in front of the C2H2.

Well, those answers are around half of the answers that I calculated. I don't understand why. Was that the whole question that you typed? Or did you simplify things and take things out, or reworded the question?

1. You've already given the molar heat of combustion of ethyne. The value is -2599 kJ/mol. As for kJ/g, you simply divide -2599 by the molar mass of ethyne. That is, -2599 / (12x2 + 2 x 1) = 99.96 kJ/g 2. Ethyne is a gas at S.T.P. Therefore there is 22.71L of gas in 1 mol of that gas. 22.71 /...

I'm not sure about the temperature, but it should be suffice to say "Heat in a water bath"... Of course there is a minimum temperature, but there is no maximum, because the reflux takes care of that. Just don't go overboard, I guess. Um, well you need boiling chips to prevent vigorous boiling...

That's weird. What if you didn't choose a lithium cell as your example? Say, like... You used button cell or something =\

Actually, I have seen a few questions that asked to calculate the pH of weak acids/bases. It is possible. Even though it isn't completely ionised and hence there will be some acid molecules that could dissociate, it would not happen, as the ionisation reaches an equilibrium. So there is no...

Doesn't matter what course they choose. But if they ace hospital/community and family studies/general maths/standard english/studies of religion, I wouldn't want to see them in a medicine course, or any other university courses that are highly demanding.

Your cohorts will become jealous of you.

Erm... Strong acid/base: Dissociates in water completely to form H+(if acid) or OH- (if base) Weak acid/base: Dissociates partially (aka incomplete dissociation of acid/base molecules)

But firstly, H2O is neither an acid nor a base. I know that under some conditions it can be regarded as a Bronsted-Lowry acid or base, but I don't think that applies here. How can you have 2 substances that are amphiprotic to react? I don't know any extra-curricular stuff, but I just reckon that...

I have no idea what you just answered. It almost seems like a foreign language. Sorry. Would you mind rewording it? Take your time while typing out your response, and read it two or three times before submitting it. A few times, I can't even figure out what you're trying to say.

Guys, don't worry about this question. This was a lame question in the CSSA, and it is very unlikely to come out in the HSC. What I have said before was the marking outline. To explain it the proper way, you'd need extra-curricular knowledge (along with most other topics as well). For now, just...