Final answer:
To calculate the number of moles of silver chromate produced from 121 g of silver nitrate, we can use the stoichiometry of the balanced chemical equation and the molar masses of the compounds involved. By setting up a proportion and solving for x, we can find the number of moles of silver chromate.
Step-by-step explanation:
To calculate the number of moles of silver chromate produced, we need to use the stoichiometry of the balanced chemical equation. The balanced equation for the reaction between silver nitrate (AgNO3) and silver chromate (Ag2CrO4) is:
2 AgNO3 + K2CrO4 ➝ Ag2CrO4 + 2 KNO3
From the equation, we can see that 2 moles of AgNO3 react to produce 1 mole of Ag2CrO4. Therefore, we can set up a proportion:
(2 moles Ag2CrO4 / 2 moles AgNO3) = (x moles Ag2CrO4 / 121 g AgNO3)
Cross-multiplying and solving for x, we find:
x = (2 moles Ag2CrO4 / 2 moles AgNO3) × (121 g AgNO3 / molar mass of AgNO3)
Finally, we need to convert grams of AgNO3 to moles using its molar mass. The molar mass of AgNO3 is obtained from the periodic table or calculated as:
molar mass of AgNO3 = atomic mass of Ag + atomic mass of N + (3 × atomic mass of O)