Question

For the following reaction, determine the amount of AgCl(s) formed when 1.046×10¹ g KCl(aq) reacts with excess AgNO₃(aq) to produce AgCl(s) and KNO₃(aq) with a 7.706×10¹% yield.

Answer 1

The amount of AgCl produced by converting the given mass of KCl to moles, applying stoichiometry based on a one-to-one reaction with AgNO3, and adjusting for the given percent yield.

Step-by-step explanation:

The question involves a stoichiometry problem where AgNO3 reacts with KCl to form AgCl and KNO3. To solve this problem, we must:

1. Convert the mass of KCl to moles using its molar mass.
2. Use the stoichiometry of the reaction to find the theoretical yield of AgCl that can be formed from the KCl.
3. Apply the percent yield to the theoretical yield to find the actual yield of AgCl.

Since the reaction between AgNO3 and KCl is one-to-one, the moles of KCl will be equal to the moles of AgCl formed. Finally, converting the moles of AgCl to grams using its molar mass and multiplying by the given percent yield gives the actual amount of AgCl produced.