Question
Use the balanced chemical equation to answer the question:
AgNO₃ + NaCl → AgCl + NaNO₃
A scientist reacts 2.4 mol of NaCl with excess AgNO₃. How many moles of each of the two products will be produced?
1.2 mol of AgCl and 2.4 mol of NaNO₃
4.8 mol of each
1.2 mol of each
2.4 mol of each
AgNO₃ + NaCl → AgCl + NaNO₃
A scientist reacts 2.4 mol of NaCl with excess AgNO₃. How many moles of each of the two products will be produced?
1.2 mol of AgCl and 2.4 mol of NaNO₃
4.8 mol of each
1.2 mol of each
2.4 mol of each
Answers
GPT-4o mini
To determine the amounts of products generated from the reaction given:
\[
\text{AgNO}_3 + \text{NaCl} \rightarrow \text{AgCl} + \text{NaNO}_3
\]
This reaction is balanced as written, with a 1:1:1:1 ratio of reactants to products.
Given that the scientist reacts 2.4 moles of NaCl with excess AgNO₃, we can analyze the reaction:
- From the balanced equation, 1 mole of NaCl produces 1 mole of AgCl and 1 mole of NaNO₃.
- Therefore, if 2.4 moles of NaCl are used, it will produce 2.4 moles of AgCl and 2.4 moles of NaNO₃.
Thus, the two products produced will be:
- 2.4 moles of AgCl
- 2.4 moles of NaNO₃
So the correct answer is **2.4 mol of each**.
\[
\text{AgNO}_3 + \text{NaCl} \rightarrow \text{AgCl} + \text{NaNO}_3
\]
This reaction is balanced as written, with a 1:1:1:1 ratio of reactants to products.
Given that the scientist reacts 2.4 moles of NaCl with excess AgNO₃, we can analyze the reaction:
- From the balanced equation, 1 mole of NaCl produces 1 mole of AgCl and 1 mole of NaNO₃.
- Therefore, if 2.4 moles of NaCl are used, it will produce 2.4 moles of AgCl and 2.4 moles of NaNO₃.
Thus, the two products produced will be:
- 2.4 moles of AgCl
- 2.4 moles of NaNO₃
So the correct answer is **2.4 mol of each**.