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 point)
Responses

2.4 mol
of each
2 point 4 mol of each

1.2 mol
of AgCl
and 2.4 mol
of NaNO3
1 point 2 mol of A g c l and 2 point 4 mol of N a N O sub 3

1.2 mol
of each
1 point 2 mol of each

4.8 mol
of each
4 point 8 mol of each
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Answer 1

To determine how many moles of each product are produced when 2.4 moles of NaCl is reacted with excess AgNO3, we can refer to the balanced chemical equation:

\[ \text{AgNO}_3 + \text{NaCl} \rightarrow \text{AgCl} + \text{NaNO}_3 \]

From this equation, we see that the reaction occurs in a 1:1:1:1 ratio. This means:

- 1 mole of AgNO3 reacts with 1 mole of NaCl to produce 1 mole of AgCl and 1 mole of NaNO3.

Since you are starting with 2.4 moles of NaCl and there is excess AgNO3, you can produce:

- 2.4 moles of AgCl (since 1 mole of NaCl produces 1 mole of AgCl)
- 2.4 moles of NaNO3 (since 1 mole of NaCl produces 1 mole of NaNO3)

Thus, the answer is:

**2.4 mol of each (AgCl and NaNO3)**.