Based on the stoichiometry of the reaction, 156.114 g of CuNO3 are required to produce 88.0 grams of aluminum nitrate, Al(NO3)3.
<h3>What is stoichiometry of a reaction?</h3>
The stoichiometry of a reaction is the molar ratio in which reactants combine to form products.
The stoichiometry of the reaction shows that 6 moles of copper (i) nitrate produces 2 moles of aluminium nitrate.
molar mass of Copper(I) nitrate, CuNO3 = 126 g
molar mass of aluminum nitrate, Al(NO3)3 = 213 g
88.0 g of aluminum nitrate, Al(NO3)3 = 88.0/213 moles = 0.413 moles
0.413 moles of Al(NO3)3 will be produced by 0.413 ×6/3 = 1.239 moles of CuNO3
Mass of 1.239 moles of CuNO3 = 1.239 × 126 = 156.114 g of CuNO3
Therefore, 156.114 g of CuNO3 are required to produce 88.0 grams of aluminum nitrate, Al(NO3)3.
Learn more about stoichiometry at: brainly.com/question/16060223
Therefore, 156.114 g of CuNO3
