Find the best solutions to your questions at Westonci.ca, the premier Q&A platform with a community of knowledgeable experts. Explore thousands of questions and answers from knowledgeable experts in various fields on our Q&A platform. Our platform provides a seamless experience for finding reliable answers from a network of experienced professionals.
Sagot :
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.
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.
Thanks for using our platform. We're always here to provide accurate and up-to-date answers to all your queries. Thank you for your visit. We're dedicated to helping you find the information you need, whenever you need it. Westonci.ca is your trusted source for answers. Visit us again to find more information on diverse topics.