I have designed a range of equivalence b/w Raoult's Law and Dalton's law in Phase Equilibria
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First you must find the submision instructions for the particular journal to which you wich to submit.  For example if you wanted to submit your work to one of the journals published by the American Chemical Society, you would start at http://pubs.acs.org/ and follow the links for submitting an article.  Once you sumbit the journal will send it through a number of reviewers who may or may not ask you questions and help you get the paper into publishable form and starndards.\n\nSome of the larger organizations have pre-print servers that allow you to upload your paper for others to consider while it awaits publication.
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Hey I'm studying physical and chemical equilibrium too, currently.The answer is that it will definitely have units when the concentrations have different powers.Just try and work it out with the units and it will be very clear.
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this requires way more than anyone can do here, but, i know of a cool java program that will do it for you: \n\nhttp://www.math.rutgers.edu/courses/ODE/sherod/phase-local.html\n\nyou can even set your initial conditions and print it out!
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While A thru C will shift the equilibrium concentrations the solubility constant will stay constant at constant temperature (at least theoretically).
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use beers law to figure out the concentration and then take that to mole ratio
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test tube- observing for chemical reations
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CH4 + 2O2-> CO2 + 2H2O
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C3H8 + 5O2 --> 3CO2 + 4H2O
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2Ca(s) + O2(g) -> 2CaO(s)
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The index-of-reaction equation (i.r.e.): dF/dtZ = kZ(l - βF)m is compared with a generalized Prout-Tompkins equation (g.P.T.e.): dF/dt = kn(l - βF)y With the boundary condition F = 0, t = 0 the equations are equivalent for z = 2 or m = 0 or β ≤ 1 and the i.r.e, is closely approximated by the g.P.T.e. for other values of the parameters by use of the following approximation ∫(1- F)-m dF ≈ AF(1-BF)5 The parameter s is a function of m. Both A and B are close to unity for 1/3 < m < 3. The i.r.e. is recommended as being more useful than the g.P.T.e. because the i.r.e. has a better theoretical basis and because it is more readily integrated and fitted to experimental data.
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To solve this problem we need to think about limiting reactants.  This one is fairly simple because I already have moles and the ratio is 1:1:1.  If I only have 3 kmols of C, that is the most I can make, because going beyond that, I would be out of C.  Thus, I can only make 3kmols of CO2 with 2 kmols of O2 left unreacted.  These amounts are theoretically find for a combustion reaction.
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It appears that the constants are calculated at one condition (dry,wet,etc) whereas the effective is closer to reality.  See\n\nhttp://www.pnas.org/cgi/content/full/102/45/16293
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Please expand on which type of "equivalents" you mean as in substitutes or normality equivalents.  For suppliers, go here:\n\nhttp://www.chemcyc.com/ME2/Default.asp
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This sounds like homework, so I'll give you the ideas but not the data.\n\nThe enthalpy of the mixture at standard conditions is the sum of standard heats of formation of the components of the mix. It will be given in kJ/mol (Ar is 0 kJ/mol being an element, the other two you can look up in tables or on internet). \n\nThen you need to adjust for the sensible energy difference compared to standard conditions : you will also need to look up the specific heat of each component (usually expressed in kJ / mol ºK) and multiply the specific heat of each component by the amount and by the difference in temperature. Make sure you have everything in the same units.\n\nRemember if you are working in moles its easier because to a first approximation, one mole of any gas occupies the same volume (if you undrestand how to allow for deviations from the ideal gas laws, you wouldn't be asking this question) and I assume that the percentages are volume percent, not by weight\n\nEnjoy
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You know three of the four things needed. Try C1V1=C2V2, or an equality.\n\n                          m/ml=m/x
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C4H9OH + 6O2 --> 4CO2 + 5H2O
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Some people might need more info. by the way.  Not everyone knows the formula for Citric Acid, and what the hell is the first equivalence point?