Calcultate the volume (in mL)of 0.250M silver nitrate solution required to react completely with a 5.00g piece of copper wire. (Assume the reaction runs at 100% yield.)
To calculate the volume of the silver nitrate solution required, we need to determine the number of moles of copper and the stoichiometry of the reaction.
1. Determine the number of moles of copper:
The molar mass of copper (Cu) is 63.55 g/mol. To convert the mass to moles, use the formula:
Moles of Copper = Mass of Copper / Molar Mass of Copper
Substituting the values, we get:
Moles of Copper = 5.00 g / 63.55 g/mol
2. Determine the stoichiometry of the reaction:
The balanced chemical equation for the reaction between silver nitrate (AgNO3) and copper (Cu) is:
2AgNO3 + Cu -> 2Ag + Cu(NO3)2
From the equation, we see that 2 moles of silver nitrate react with 1 mole of copper.
3. Calculate the moles of silver nitrate required:
Since the stoichiometry shows that 2 moles of silver nitrate react with 1 mole of copper, the moles of silver nitrate needed can be calculated as:
Moles of AgNO3 = Moles of Copper / 1 * 2
Substituting the values, we get:
Moles of AgNO3 = (5.00 g / 63.55 g/mol) * 2
4. Calculate the volume of the silver nitrate solution:
The concentration of the silver nitrate solution is given as 0.250 M, which means there are 0.250 moles of silver nitrate per liter of solution (1000 mL).
To convert the moles of silver nitrate to volume, use the formula:
Volume of AgNO3 = Moles of AgNO3 / Concentration of AgNO3
Substituting the values, we get:
Volume of AgNO3 = (5.00 g / 63.55 g/mol) * 2 / 0.250 M
5. Convert the volume to mL:
The calculated volume is in liters, but we need to express it in milliliters. Since there are 1000 mL in 1 L, multiply the volume in liters by 1000 to get the volume in mL:
Volume of AgNO3 in mL = Volume of AgNO3 * 1000
Calculating these values will give you the volume of the 0.250 M silver nitrate solution required to react completely with the 5.00 g piece of copper wire.
Here is an example. Just follow the steps.
http://www.jiskha.com/science/chemistry/stoichiometry.html
The equation is
2Ag+(aq) + Cu(s) ==> Cu2+(aq) + 2Ag(s)