Question

Given the following reaction:

Cu + 2AgNO3 → 2Ag + Cu(NO3)2
How many grams of Ag will be produced from 5.00 g of Cu and 1.00 g of AgNO3?

Answer 1

0.648 g of Ag ( silver) is produced

Step-by-step explanation:

First calculating the moles of the reactants given;

Cu = 5/64 = 0.078 moles

Mr ( molecular mass) of AgNO3 = 108 + 14 + (16 x 3)

= 170 g

Now the moles of AgNO3 ;

1/170 = 0.006 moles

setting up mole ratio to calculate the limiting reactant:

moles of Cu : moles of Ag

1 : 2

0.078 : X

X = 0.078 x 2

= 0.156 moles of Ag

moles of AgNO3 : moles of Ag

2 : 2

0.006 : X

X = (0.006 x 2)/2

= 0.006 moles of Ag

As silver nitrate ( AgNO3) gives the least number of moles of Ag therefore it is the limiting reactant and would control the amount of product formed.

Now the mass of Ag formed:

atomic mass x moles

= 108 x 0.006

= 0.648 g of Ag ( silver) is produced