Question

What is the mass of silver that can be prepared from 1.50 g of copper metal?

Cu(s)+2AgNO3(aq)→Cu(NO3)2(aq)+2Ag(s)

Answer 1

Molar mass:

Ag = 107.86 g/mol
Cu = 63.54 g/mol

Mole ratio:

Cu(s)+2 AgNO₃(aq)→Cu(NO₃)₂(aq)+2 Ag(s)

63.54 g Cu ------------- 2 x 107.86 g Ag
1.50 g Cu -------------- ??

Mass Ag = 1.50 x 2 x 107.86 / 63.54

Mass Ag = 32358 / 63.54

= 509.25 g of Ag

hope this helps!

Answer 2

The mass of silver that can be prepared from 1.50 g of copper metal is 5.10 g.

To find the mass of silver that can be prepared from 1.50 g of copper metal, we need to use stoichiometry and the balanced chemical equation.

From the equation, we can see that 1 mole of copper reacts with 2 moles of silver to produce 1 mole of copper(II) nitrate and 2 moles of silver.

We can use the molar masses of copper and silver to convert grams to moles, and then use the mole ratio to find the moles of silver. Finally, we can convert moles of silver back to grams using the molar mass of silver.

Step 1: Convert grams of copper to moles of copper. (1.50 g Cu) / (63.55 g/mol Cu) = 0.0236 mol Cu

Step 2: Use the mole ratio of silver to copper from the chemical equation. (0.0236 mol Cu) × (2 mol Ag / 1 mol Cu) = 0.0473 mol Ag

Step 3: Convert moles of silver to grams of silver. (0.0473 mol Ag) × (107.87 g/mol Ag) = 5.10 g Ag