Question

Cu+2AgNO

3

​

→2Ag+Cu(NO

3

​

)

2

​

start text, C, u, end text, plus, 2, start text, A, g, N, O, end text, start subscript, 3, end subscript, right arrow, 2, start text, A, g, end text, plus, start text, C, u, left parenthesis, N, O, end text, start subscript, 3, end subscript, start text, right parenthesis, end text, start subscript, 2, end subscript

How many grams of \text{Ag}Agstart text, A, g, end text will be produced from 19.0 \text{ g}19.0 g19, point, 0, start text, space, g, end text of \text{Cu}Custart text, C, u, end text and 125 \text{ g}125 g125, start text, space, g, end text of \text{AgNO}_3AgNO

3

​

start text, A, g, N, O, end text, start subscript, 3, end subscript?

Answer 1

Answer:

Mass of Ag produced = 64.6 g

Note: the question is, how many grams of Ag is produced from 19.0 g of Cu and 125 g of AgNO3

Explanation:

Equation of the reaction:

Cu + 2AgNO3 ---> 2Ag + Cu(NO3)2

From the equation above, 1 mole of Cu reacts with 2 moles of AgNO3 to produce 2 moles of Ag and 1 mole of Cu(NO3)2.

Molar mass of the reactants and products are; Cu = 63.5 g/mol, Ag = 108 g/mol, AgNO3 = 170 g/mol, Cu(NO3)2 = 187.5 g/mol

To determine, the limiting reactant;

63.5 g of Cu reacts with 170 * 2 g of AgNO3,

19 g of Cu will react with (340 * 19)/63.5 g of AgNO3 =101.7 g of AgNO3.

Since there are 125 g of AgNO3 available for reaction, it is in excess and Cu is the limiting reactant.

63.5 g of Cu reacts to produce 108 * 2 g of Ag,

19 g of Cu will react to produce (216 * 19)/63.5 g of Ag = 64.6 g of Ag.

Therefore mass of Ag produced = 64.6g