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C3 pages 127-128 (concentrations of solutions (concentration (mass of…
C3 pages 127-128
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limiting reactants
when some magnesium carbonate is placed in a beaker of hydrochloric acid, you can tell a reaction is taking place because you can see lots of bubbles of gas being given off. after a while the fizzing slows down and eventually stops
the reactant stops when all of one of the reactants is used up any other reactants are in excess. they are usually added in in excess to make sure that the other reactant is used up
the reactant that's used up in a reaction is called the limiting reactant because it limits the amount of product that's formed.
the amount formed is directly proportional to the amount limiting reactant. for example if you half the amount of limiting reactant the amount of product formed will also half. if you double the amount of limiting reactant the amount of product will double (as long as its still the limiting reactant)
this is because if you add more reactant there will be more reactant particles to take part in the reaction, which means more product particles.
you can calculate the mass of a product formed in a reaction by using the mass of the limiting reactant and the balanced reaction equation
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4) use the balanced equation to work out how many moles there'll be of the other substance. in this case that's how many moles of the product will be made of this many moles of reactant
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reactions don't go on forever. If one reactant gets completely used up in a reaction before the rest, the reaction will stop. this reactant is limiting.