madey21
Answered

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Given the balanced chemical equation:
[tex]\[ \text{AgNO}_3 + \text{NaCl} \rightarrow \text{AgCl} + \text{NaNO}_3 \][/tex]

75.0 mL of 0.500 M \(\text{AgNO}_3\) reacts with 35.0 mL of 1.00 M \(\text{NaCl}\). How many moles of \(\text{AgCl}\) can form from the \(\text{NaCl}\)?

[tex]\[
\frac{0.0350 \, \text{L} \, \text{NaCl}}{1} \times \frac{1.00 \, \text{mol} \, \text{NaCl}}{1 \, \text{L}} \times \frac{1 \, \text{mol} \, \text{AgCl}}{1 \, \text{mol} \, \text{NaCl}} =
\][/tex]

Sagot :

GinnyAnswer
To determine how many moles of AgCl can form from the given amount of NaCl, we can follow the steps outlined below:

1. Convert the volume of NaCl solution from milliliters to liters:
Given that the volume of NaCl solution is 35.0 mL, we need to convert this to liters:
[tex]\[ 35.0 \text{ mL} = 35.0 \text{ mL} \times \left(\frac{1 \text{ L}}{1000 \text{ mL}}\right) = 0.0350 \text{ L} \][/tex]

2. Determine the moles of NaCl:
Knowing the molarity (concentration) of the NaCl solution is 1.00 M (moles per liter), we can find the moles of NaCl present:
[tex]\[ \text{Moles of NaCl} = \text{volume in liters} \times \text{molarity} = 0.0350 \text{ L} \times 1.00 \text{ M} = 0.035 \text{ moles of NaCl} \][/tex]

3. Determine the moles of AgCl formed:
From the balanced chemical equation,
[tex]\[ \text{AgNO}_3 + \text{NaCl} \rightarrow \text{AgCl} + \text{NaNO}_3 \][/tex]
we see that 1 mole of NaCl reacts with 1 mole of AgNO₃ to produce 1 mole of AgCl. Therefore, the moles of AgCl formed will be equal to the moles of NaCl reacted.

So, the moles of AgCl formed from the moles of NaCl is:
[tex]\[ 0.035 \text{ moles of AgCl} \][/tex]

Hence, from 35.0 mL of 1.00 M NaCl, [tex]\(0.035\)[/tex] moles of [tex]\( \text{AgCl} \)[/tex] can form.
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