rate and extent of chemical reation?
824613
Rate of chemical reactions depend on - temperature, pressure, concentration and the use of catalyst. The rxn constant (generally used in equilibriums) is often calculated to able to see the rate of the reaction. \n\nX + Y <----> 2V + Z\n\neq constant =  ([V^2]x[Z])/[X]x[Z]) \n\nThe higher the constant, the higher the rate. Equilibrium constant only changes if the there's a temperature change. Concentration changes doesn't effect the constant however it effects the rate. Although pressure changes lead to temperature changes, it's assumed that pressure changes don't effect the constant. If the constant is greater than 10^6, rxn will take place at reasonable rate.
97267
I think you mean "chemistry"... I don't know any sites off hand but you can always just try a search engine, like Yahoo and search for chemistry.\nOr is there something called "chemestry" that I don't know about yet.
753451
A bit vague but a you could work out the rate from a titration, also the molar value from the same experiment.
370859
Presuming that bromine is getting reduced to Br(-) and bisulfite is getting oxidized to sulfate (not including the spectator sodium ion):\n\nReduction half-reaction\nBr2 + 2e ---->  2Br(-)\n\nOxidation half reaction\nHSO3(-) + H2O ----->  SO4(2-) + 2e + 3H(+)\n\nOverall Reaction:\nBr2 + HSO3(-) + H2O ---->  SO4(2-) + 2Br(-) + 3H(+)
1102790
http://www.chem.uni-potsdam.de/~thomas/1hbuch/english/index.html\n\nhere is a website that seems short and simple\ngood luck
230380
um i don't know if this site has it, but you might want to try chemguide.co.uk :) it's a pretty good site.
84780
!!!!!!!!!!!!!!!! \nI think rather u wanted to ask how can u predict the formula of a chemical reaction!!\nFirstly, we have to determine the moles of reactant taking part.(It can be done easily, think A reacts with B, just mix 1 mole of A with the same amount of B.)\nThen determine what are the different products and their amounts.\nAll u have to do is some calculations..................\nRemember its not as easy as it sounds.
679000
time= 2.303/(rate constant) log( initial conc / final conc)\n\nthis is for a first order reaction...
729117
You don't give the rate law, so it's impossible to tell. Suppose [H2O2] = concentration of H2O2 and [I-] = concentration of iodide. If rate = k[H2O2][I-], then the mechanism is one step. This means that both an H2O2 and an I- have to come together at the same time for the reaction to occur. If rate = k[H2O2], then it's a two-step process. This is because something has to happen to H2O2 in a slow, rate-limiting step, followed by the reaction of whatever with I-.
598319
http://www.sbuniv.edu/~ggray/CHE3345/chp14.html\nhttp://web.odu.edu/sci/tisenhou/chem321/chap12/index.htm\n\nbest luck
383259
go to\nwww.chemistry.com
940690
that would depend on the molarity of the substance. there could be any number of moles in that much solution.
963470
CO + 2H2  --->  CH3OH\n\nmoles H2: 2.00g/ 1g/mol = 2.00 mol\nmoles CO: 18.50g / 28g/mol = 0.6607mol\n\nyour limiting reactant is CO since for every 0.6607 moles of CO, you'll only need 1.321 moles H2. there's an excess of 0.6790 moles H2.\n\ntheoretical yield, therefore, is (1.321/2)*100 =  66.05%\n\nbased from the balanced equation, there should also be 0.6607 moles of CH3OH (MW = 32g/mol) that will be formed. so,\n\nweight of CH3OH = 0.6607mol * 32g/mol = 21.14 grams
974075
the larger the size, the greater the surface area, the greater the reaction rate.\n\nsize is the independent variable, the rate of the reaction depends on the size, so rate is the dependent variable
718831
Try chemdex.\n\nhttp://www.chemdex.org/
842465
you could call it something like "rate of reaction"
618961
6 moles of hydrochloric acid will react at a faster rate than 1 mole of hydrochloric acid because the solution will not dilute as fast as the smaller amount of acid- more acid to react with the Zinc.\n\nSounds good to me...