Calculate the mass of silver metal (Ag) produced from the reaction of 5.58 grams of copper metal (Cu) according to the following reaction:
Cu(s) + 2AgNO3(aq) --> Cu(NO3)2(aq) + 2Ag(s)
Here is a sample. Just follow the steps.
http://www.jiskha.com/science/chemistry/stoichiometry.html
To calculate the mass of silver (Ag) produced, you need to use stoichiometry. Stoichiometry allows you to relate the amounts of reactants and products in a chemical equation.
First, you need to determine the molar mass of copper (Cu) and silver (Ag).
The molar mass of Cu is 63.55 g/mol, and the molar mass of Ag is 107.87 g/mol.
Next, you need to determine the balanced chemical equation for the reaction and use it to determine the stoichiometry ratio between copper and silver. From the reaction given, you can see that for every 1 mole of Cu, 2 moles of Ag are produced.
Now it's time to do the math. Start by converting the mass of Cu given (5.58 grams) to moles using its molar mass.
moles of Cu = mass of Cu / molar mass of Cu
moles of Cu = 5.58 g / 63.55 g/mol = 0.0877 mol
Now, using the stoichiometry ratio from the balanced equation, you can determine the moles of Ag produced.
moles of Ag = moles of Cu * (2 moles of Ag / 1 mole of Cu)
moles of Ag = 0.0877 mol * (2/1) = 0.1754 mol
Finally, convert moles of Ag to grams by multiplying by the molar mass of Ag.
mass of Ag = moles of Ag * molar mass of Ag
mass of Ag = 0.1754 mol * 107.87 g/mol = 18.91 grams
Therefore, the mass of silver (Ag) produced from the reaction of 5.58 grams of copper (Cu) is approximately 18.91 grams.