7) You have a 2.5M solution of Silver Nitrate. It contains 450mL of solution. How many grams of silver would you be able to extract?
Cu (s) + 2AgNO3 (aq) -> 2Ag (s) + Cu (NO3)2 (aq)
I've gotten this much:
M=mol/L
2.5=mol/.45
mol= 2.5*.45
mol=1.125
Silver Nitrate= (Ag=107.9)+(N=14.01)+(O=16.00*3) = 169.91*1.125= 191.148
I know the answer is 121.3, but I don't know how to get there
Thanks!
To calculate the mass of silver that can be extracted from the solution, you need to determine the number of moles of silver present in the solution and then convert it to grams.
1. Calculate the number of moles of silver nitrate:
- Given that the molarity (M) is 2.5 M and the volume (V) is 450 mL (or 0.45 L), you can use the formula M = mol/L to find the moles.
- Rearrange the equation to solve for moles: mol = M × L = 2.5 mol/L × 0.45 L = 1.125 mol
2. Determine the molar mass of silver nitrate:
- The molar mass of silver nitrate (AgNO3) can be calculated by adding up the atomic masses of its constituent atoms.
- AgNO3 consists of one Ag atom (with an atomic mass of 107.9 g/mol), one N atom (with an atomic mass of 14.01 g/mol), and three O atoms (each with an atomic mass of 16.00 g/mol).
- Calculate the molar mass: 107.9 g/mol + 14.01 g/mol + (16.00 g/mol × 3) = 169.91 g/mol
3. Calculate the mass of silver:
- To find the mass of silver, multiply the moles of silver nitrate by the molar mass of silver:
- Mass of silver = moles of silver nitrate × molar mass of silver
- Mass of silver = 1.125 mol × 169.91 g/mol = 190.909 g
Therefore, you would be able to extract approximately 190.909 grams of silver from the 2.5M solution of Silver Nitrate. Rounded to one decimal place, the mass would be approximately 190.9 grams.
To calculate the amount of silver that can be extracted from the solution of silver nitrate, we need to determine the number of moles of silver nitrate present in the solution and then use the stoichiometry of the reaction to find the moles of silver produced.
Let's break down the steps:
1. Convert the given volume of the solution from milliliters (mL) to liters (L):
450 mL = 450/1000 = 0.45 L
2. Calculate the number of moles of silver nitrate:
Molarity (M) = moles of solute / liters of solution
Rearranging the equation, moles of solute = Molarity × liters of solution
Moles of silver nitrate = 2.5 M × 0.45 L = 1.125 moles
3. Use the stoichiometry of the reaction to find the moles of silver produced:
From the balanced equation, we can see that 2 moles of silver nitrate produce 2 moles of silver (Ag).
So, moles of silver = 1.125 moles × (2 moles Ag / 2 moles AgNO3) = 1.125 moles
4. Calculate the mass of silver using the molar mass of silver (Ag):
Molar mass of silver (Ag) = 107.9 g/mol
Mass of silver = moles of silver × molar mass of silver = 1.125 moles × 107.9 g/mol = 121.3 grams
Therefore, you would be able to extract 121.3 grams of silver from the given solution of silver nitrate.