hermanntrude

burning parsley smells EXACTLY like burning marijuana

you should be careful with that one. it's an antique

how rediculously large? you said yourself that the assumption isn't true, and have you ever seen a champagne cork go off? it really moves. that's because of high pressure.

here's a useful link

there is a dwarf planet called makemake (snigger)

I used to know a forum-goer called SCB... it stood for stone cold bitch... that's not you, i'm guessing. she would have made more of an entrance... she was a dominatrix

I think perhaps it works better if you stop backseat modding and just imagine the title of the thread to be something a bit broader "general discussion of home chemistry" perhaps?

I'd recommend more than just caution here. I'd recommend NOT DOING it. very strongly recommend.

here's a good link

the plural of octopus is octopodes. NOT octopusses or octopussies or octopi.

What exactly do you want to hear? if you want our permission or agreement on your chosen method, you won't get it. Our hazmat policy doesnt allow us to recommend a dangerous procedure. I've used chlorine myself but i have a fume hood, and even then it gave me a sore throat for a day or so. And as UC said, you'd still end up with a nasty mixture which will be hard to separate. Give it up and buy some. buy a chemistry set... they always have KMnO4 in them anyway.

hmm well i'm not sure how violent the reaction might be... it is a mixture of a fairly strong oxidising agent and a reducing agent

also good is sparknotes

is an essential oil a single substance or a mixture?

also read this This document is something you shoudl be famliar with if you work with chemicals ever, even just at home for fun. It's called a material safety data sheet and contains all the things you need to know before using a chemical. The one for chlorine is quite startling. it's very dangerous stuff.

there's a quicker way to answer this without calculus, too: mathworld says that the volume of a spherical ring is equal to [math]V = \frac{4}{3}(r^2-R^2)^\frac{3}{2}[/math] where r is the radius of the drilled hole and R is the radius of the sphere Interestingly you can also get the volume of the spherical ring knowing only the length of the hole: [math] V = \frac{1}{6}\pi L^3[/math] where L is the length of the hole (measured after drilling... in other words not including the depth of the spherical caps.)

OK the first step you need to take is to find an equation which actually has methane in it. The only candidate is the third one: [ce]CH4 + 2O2 -> CO2 + 2H2O[/ce] [math]\Delta H = -895 kJmol^{-1}[/math] The only problem with this equation is it has methane as a reactant rather than a product. You need to turn it around. What happens to the enthalpy of a reaction when you run it backwards? [ce]CO2 + 2H2O -> CH4 + 2O2[/ce] [math]\Delta H[/math] = ??? I'll leave it for you to find out what to do to get the enthalpy for this reaction. Then you need to find equations which have carbon and hydrogen as reactants (remember that a heat of formation is the enthalpy associated with the formation of a substance from its elements, in this case, carbon and hydrogen). The first two equations look good to me: [ce] H2 + 1/2O2 -> H2O[/ce] [math]\Delta H = -280 kJmol^{-1}[/math] and [ce] C + O2 -> CO2[/ce] [math]\Delta H = -393 kJmol^{-1}[/math] The only problem now is that we want 4 moles of hydrogen and we've only got two. So we need to double the first equation: [ce] 2H2 + O2 -> 2H2O[/ce] [math]\Delta H = ???[/math] Again, i'll leave it to you to figure out what needs to be done to the enthalpy when you double the equation. Finally, you can add them all together to get the equation we've been looking for: [ce] 2H2 + O2 -> 2H2O[/ce] [math]\Delta H = ???[/math] [ce] C + O2 -> CO2[/ce] [math]\Delta H = -393 kJmol^{-1}[/math] [ce]CO2 + 2H2O -> CH4 + 2O2[/ce] [math]\Delta H[/math] = ??? total: [ce]2H2 + 2O2 + C + CO2 + 2H2O -> 2H2O + CO2 + 2O2 + CH4[/ce] [ce]2O2[/ce], [ce]CO2[/ce], and [ce]H2O[/ce] all appear on both sides, so they can be cancelled: [ce]2H2 + C -> CH4[/ce] You can get the enthalpy for this by simply adding the enthalpies of the equations you added together to make it. This is an example of Hess's law, which I recommend you read up on. I hope this helps. If not, please ask me a specificly worded question IN THIS THREAD (not a new one). Thanks.

shut up

If UC is correct in his assumption, you've answered the question pretty well. One suggestion I'd make is to write that it causes an apparent increase in the percentage yield. because of course it hasnt changed how much copper you've got at all.

certain chemicals when added to water can cause the water to heat up or cool down. For instance, if you add sodium hydroxide to water, the water can often boil if you add enough.

excel can do that too... but you have to use a function to calculate it

I'd probably wash it with ethanol of acetone, then put it in a dessicator with a dessicating agent and NaOH

because if they didnt, stars would get in the way when you were trying to read

although you have to be enormously careful with what you smell. For instance, cyanides smell of almonds, but usually only very briefly...