How many atoms of silver would be produced if 100 grams of copper reacts with an excess of silver nitrate cu + 2 agno3 -> cu(no3)2 + 2 ag

the balanced equation for the above reaction is as follows

Cu + 2AgNO₃ ---> Cu(NO₃)₂ + 2Ag

stoichiometry of Cu to Ag is 1:2

the limiting reactant is the reactant that is fully used up in the reaction. the amount of product formed depends on amount of limiting reactant present

Copper reacts with excess silver nitrate therefore Copper is the limiting reactant

mass of copper reacted - 100 g

number of moles of copper reacted - 100 g / 63.5 g/mol = 1.57 mol

according to stoichiometry number of Ag moles formed - number of copper moles x 2

number of Ag moles formed - 1.57 x 2 = 3.14 mol

1 mol of Ag is made of 6.022 x 10²³ atoms of Ag

therefore 3.14 mol of Ag is made of - 6.022 x 10²³ atoms/mol x 3.14 mol = 1.89 x 10²⁴ atoms

1.89 x 10²⁴ atoms of Ag are formed in the reaction

explanation: it gains negative electrons, therefore becoming negatively charged. as charge cannot be created, nor destroyed, only transferred, this leaves the wool positive. now that they have opposite charges, the two items attract.