Answered




In the reaction K2CrO4(aq) + PbCl2(aq) → 2KCl(aq) + PbCrO4(s), how many grams of PbCrO4 will precipitate out from the reaction between 500.0 milliliters of 3.0 M K2CrO4 in an excess of PbCl2?


1.5 grams


3.0 grams


480 grams


150 grams

Verified Answer :

taskmasters

The balanced chemical reaction is:

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. 


3.0 M K2CrO4 (.500 L) = 1.5 mol K2CrO4

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


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

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