Answer :
The reagent that is in excess in this experiment is potassium dichromate (K2CrO4).
To determine which reagent is in excess, we need to calculate the moles of each reagent and compare them.
Moles of AgNO3 = 0.0040 M x 0.0050 L = 2.0 x 10^-5 moles
Moles of K2CrO4 = 0.0024 M x 0.0050 L = 1.2 x 10^-5 moles
Since the moles of AgNO3 is greater than the moles of K2CrO4, we might initially think that AgNO3 is in excess. However, we need to consider the balanced chemical equation for the reaction:
AgNO3 + K2CrO4 → Ag2CrO4 + 2KNO3
From the balanced equation, we can see that 1 mole of AgNO3 reacts with 1 mole of K2CrO4. Therefore, we only need 1.2 x 10^-5 moles of AgNO3 to react completely with the 1.2 x 10^-5 moles of K2CrO4. Since we added 2.0 x 10^-5 moles of AgNO3, we have an excess of AgNO3.
Therefore, the reagent that is in excess is the potassium dichromate (K2CrO4).
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