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o-na [289]
3 years ago
11

In the reaction K2CrO4(aq) + PbCl2(aq) → 2KCl(aq) + PbCrO4(s), how many grams of PbCrO4 will precipitate out from the reaction b

etween 500.0 milliliters of 3.0 M K2CrO4 in an excess of PbCl2?
1.5 grams

3.0 grams

480 grams

150 grams
Chemistry
1 answer:
Elodia [21]3 years ago
7 0
The balanced chemical reaction is:

<span>K2CrO4(aq) + PbCl2(aq) → 2KCl(aq) + PbCrO4(s)

We are given the amount of the reactants to be used for the reaction. These amounts will be the starting point of our calculations. </span>

<span>
3.0 M K2CrO4 (.500 L) = 1.5 mol K2CrO4

</span>1.5 mol K2CrO4 (1 mol PbCrO4 / 1 <span>mol K2CrO4</span>) ( 323.2 g/mol)=484.8 grams PbCrO4


Therefore, the best answer from the choices is 480 grams.

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