This is a limiting regent (LR) problem. You know that when amounts are given for BOTH reactants.
mols AgNO3 = M x L = ?
mols K2C4O4 = M x L = ?
Using the coefficients in the balanced equation convert mols AgNO3 to mols Ag2CrO4
Do the same for mols K2CrO4 to mols Ag2CrO4
It is likely that these two values for mols Ag2CrO4 don't agree which means one is not right. The correct value in LR problems is ALWAYS the smaller value and the reagent producing that value is the LR.
Now take the smaller value of mols and convert to grams. g = mols x molar mass
Silver chromate may be prepared by the following reaction.
2 AgNO3(aq) + K2CrO4(aq) Ag2CrO4(s) + 2 KNO3(aq)
Calculate the mass of silver chromate produced when 0.623 L of 1.345 M silver nitrate is reacted with 245 mL of 1.89 M potassium chromate.
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