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Based on the coefficients in a given a balanced equation, a certain ratio must exist between reactants in order to obtain a certain amount of product. This ratio is the mole ratio we discussed previously
However, now suppose that you simply want to make as much product as possible given the amounts of reactant you currently have. Suppose also that the amount of each reactant you have is not in the correct ratio. You find that you have an almost endless supply of the first of your two reactants, but very little of the second. What happens? Well, obviously, you are not going to be able to use all of the first reactant. It will only combine in ratio with the second; the excess will have nothing to react with. The amount of product you obtain will therefore be in ratio with the second reactant. Confused? An example is long overdue.
Problem: You have 10 g of solid carbon, but only 10 mL of pure oxygen
gas. Not all of the carbon will be used in the reaction. Given that the
reactants react according the following balanced equation, how many molecules of
CO2(g) can be produced? How many grams of C(s) will react?
How much C(s) is left over after all the oxygen is gone?
C(s) + O2(g)→CO2(g) |
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10 grams C(s) -5.352×10-3 grams C(s) = 9.995 grams C(s) |
Now, in the example problem, we were more or less told which reactant was the
limiting reagent. However, many times you will have to figure this out.
Problem: Salt (sodium chloride) is prepared by the reaction of sodium
metal with chlorine gas.
2Na(s) + Cl2(g)→2NaCl(s) |
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