Can u show the solution to this problem? What is the mass of silver that can be prepared for 1.00g of copper metal Cu (s)+2AgNO3(ag)= Cu(NO3)2(ag)+2Ag(s)
To determine the mass of silver that can be prepared from 1.00g of copper metal, we need to use stoichiometry and the given balanced chemical equation:
Cu (s) + 2AgNO3 (ag) → Cu(NO3)2 (ag) + 2Ag (s)
1. Begin by identifying the molar mass of copper (Cu) and silver (Ag). The molar mass of Cu is 63.55 g/mol, and Ag is 107.87 g/mol.
2. Determine the number of moles of Cu in 1.00g of copper using the formula:
moles = mass / molar mass
moles of Cu = 1.00g / 63.55 g/mol
3. Apply stoichiometry to determine the number of moles of Ag that can be produced. From the balanced chemical equation, we know that the mole ratio of Cu to Ag is 1:2.
moles of Ag = moles of Cu * (2 moles of Ag / 1 mole of Cu)
4. Calculate the mass of Ag using the formula:
mass = moles * molar mass
mass of Ag = moles of Ag * 107.87 g/mol
By following these steps, you will be able to calculate the mass of silver that can be prepared from 1.00g of copper metal.