How many grams of cadmium must react to displace 13.0 g of copper from a solution of copper nitrate?

Cu(NO3)2 + Cd ==> Cd(NO3)2 + Cu

Just follow the steps in this stoichiometry problem I've posted.
http://www.jiskha.com/science/chemistry/stoichiometry.html

To determine how many grams of cadmium are needed to displace a certain amount of copper, we need to calculate the stoichiometry of the reaction using balanced chemical equations and molar masses.

First, let's write the balanced chemical equation for the reaction between cadmium and copper nitrate:

Cd + Cu(NO3)2 → Cd(NO3)2 + Cu

From the balanced equation, we can see that 1 mole of cadmium reacts with 1 mole of copper nitrate to produce 1 mole of cadmium nitrate and 1 mole of copper.

Next, we need to determine the molar masses of copper (Cu) and cadmium (Cd). The molar mass of copper is approximately 63.55 g/mol, and the molar mass of cadmium is approximately 112.41 g/mol.

Using the molar masses, we can now set up a proportion to calculate the number of moles of copper in 13.0 g of copper.

13.0 g Cu * (1 mol Cu / 63.55 g Cu) = 0.204 mol Cu

Since we know from the balanced equation that 1 mole of cadmium reacts with 1 mole of copper, we can conclude that 0.204 moles of cadmium are needed to displace 0.204 moles of copper from the solution.

Finally, we can convert the moles of cadmium into grams.

0.204 mol Cd * (112.41 g Cd / 1 mol Cd) = 22.93 g Cd

Therefore, approximately 22.93 grams of cadmium must react to displace 13.0 grams of copper from the copper nitrate solution.