Question

If you combine 15.5 g of silver nitrate and 12.1 g of potassium chromate , determine the limiting reactant, masses of products, and mass of excess reactant.

The following 7 questions will be based on this reaction.
MM silver nitrate = 169.88 g/mol
MM potassium chromate = 194.20 g/mol
MM silver chromate = 331.74 g/mol
MM potassium nitrate = 101.11 g/mol
1. Based upon the above reaction, write the balanced chemical equation for the reaction.
2. Show the calculation of the 1st reaction beginning with silver nitrate and ending with amount of product of silver chromate produced. Put the amount in below.
3. Show the calculation of the 2nd reaction beginning with potassium chromate and ending with amount of product of silver chromate produced. Put the amount in below.
4. Based on the answer to the questions above, the limiting reactant is ____?
5. Based on the answers to the questions above, what is the amount of silver chromate made by this reaction?
6. In your pdf, show the calculation of the 3rd reaction beginning with the limiting reactant and ending with amount of potassium nitrate that can be made. Put that value in below.
7. In your pdf, show how you determined the amount of the excess reactant left over. Put that value in below.

Answer 1

Step-by-step explanation:

To determine the limiting reactant,

compare the moles of AgNO3 (0.091) and K2CrO4 (0.062).

As the ratio (1.468) is less than 2:1, K2CrO4 is limiting. The theoretical yield of Ag2CrO4 is 0.062 moles * 331.87 g/mol. The mass of excess AgNO3 is 15.5 g - (0.062 moles * 169.87 g/mol).

Now you can calculate the theoretical yield of Ag2CrO4 and the mass of excess AgNO3 using the given values.