Calcium chloride (CaCl2) and silver nitrate (AgNO3) react to form calcium nitrate (Ca(NO3)2) and silver chloride (AgCl) according to the following balanced equation:
CaCl2 + AgNO3 → Ca(NO3)2 + AgCl
In order to find the number of moles of calcium chloride required to react with 350 grams of silver nitrate, we can use the concept of stoichiometry. Stoichiometry is the study of the quantitative relationships between the reactants and products in a chemical reaction. By using the balanced equation and molar masses of the reactants and products, we can calculate the number of moles of one substance required to react with a certain number of moles of another substance.
Here's the step by step process:
Determine the molar mass of silver nitrate (AgNO3). The molar mass of AgNO3 is 169.87 grams/mole.
Convert the given mass of silver nitrate to moles. To do this, divide the mass by the molar mass:
350 grams AgNO3 / 169.87 grams/mole = 2.05 moles AgNO3
Use the stoichiometry of the balanced equation to determine the number of moles of calcium chloride required to react with 2.05 moles of silver nitrate. The coefficients in the balanced equation indicate the molar ratios between the reactants and products. In this case, the coefficients are 1:1, meaning that for every 1 mole of calcium chloride that reacts, 1 mole of silver nitrate also reacts. Therefore, the number of moles of calcium chloride required is 2.05 moles.
In conclusion, to react with 350 grams of silver nitrate, we need 2.05 moles of calcium chloride.