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

answer: the value of enthalpy change will be -152.80 kj.

solution:

pressure = 1atm , temperature = = 298 k

given that pressure and temperature are same in both gases , the number of moles of both gases can be determined by the ideal gas equation.

according to reaction 3 moles no are reacting with 1 mol of ,then 0.49 mol of no will react with moles of ozone that is 0.16 moles of ozone. since, no is limiting reagent and is an excessive reagent.

enthalpy change for the reaction between the given volumes of the gases is :

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