How many moles of silver will be deposited from a silver (i) trioxonitrate (v) solution by 16.0g of copper (Ag=108,Cu=63.5)

Question

Create a beautiful and insightful illustration showcasing the process of a chemical reaction with the focus on the use of silver trioxonitrate solution and copper. The illustration should depict the weight ratios of 16.0g of copper in relation to a theoretical amount of silver (Ag=108,Cu=63.5). Include visual representations of silver, copper, and a trioxonitrate solution, as well as the change within the reaction process. Remember, the image should not contain any text.

How many moles of silver will be deposited from a silver (i) trioxonitrate (v) solution by 16.0g of copper (Ag=108,Cu=63.5)

Answer 1

I wonder why you don't call that silver nitrate?

2AgNO3 + Cu --> Cu(NO3)2 + 2Ag
mols Cu = grams/atomic mass = ?
Then you get 2 mols Ag for every mol of Cu.

Answer 2

Well, let's get this chemistry party started! To determine the number of moles of silver that will be deposited, we need to use stoichiometry. It's like a chemical party trick!

So, first things first, we need to balance the equation. The reaction between silver (Ag) and copper (Cu) can be represented as:

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

From the equation, we can see that 2 moles of silver are produced for every 1 mole of copper.

Now, let's calculate the number of moles of copper in 16.0g of copper. To do this, we need to divide the mass of copper by its molar mass:

16.0g Cu * (1 mol Cu / 63.5g Cu) = 0.252 mol Cu

Since the stoichiometry of the reaction tells us that 1 mole of copper results in 2 moles of silver, we can multiply the moles of copper by the stoichiometric ratio:

0.252 mol Cu * (2 mol Ag / 1 mol Cu) = 0.504 mol Ag

So, approximately 0.504 moles of silver will be deposited from the silver (I) trioxonitrate (V) solution by 16.0g of copper. That's a whole lot of silver! Let's start a jewelry business! 🤡💍

Answer 3

To determine the number of moles of silver (Ag) that will be deposited from a silver (I) trioxonitrate (V) solution by 16.0g of copper (Cu), we need to use the balanced chemical equation for the reaction between copper and silver nitrate:

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

From the balanced equation, we can see that 2 moles of Ag will be produced for every mole of Cu consumed.

Now, let's calculate the number of moles of Cu:

Given:
Mass of Cu = 16.0g
Molar mass of Cu = 63.5g/mol

Number of moles of Cu = Mass / Molar mass
Number of moles of Cu = 16.0g / 63.5g/mol ≈ 0.252 moles of Cu

Since the reaction has a 1:2 ratio between Cu and Ag, the number of moles of Ag deposited will be twice the number of moles of Cu:

Number of moles of Ag = 2 * Number of moles of Cu
Number of moles of Ag = 2 * 0.252 moles ≈ 0.504 moles of Ag

Therefore, approximately 0.504 moles of silver will be deposited from the silver (I) trioxonitrate (V) solution by 16.0g of copper.

Answer 4

To find the number of moles of silver that will be deposited, we need to use the concept of stoichiometry and the balanced chemical equation for the reaction between copper and silver trioxonitrate.

The balanced equation for the reaction is:
3Cu + 8AgNO3 → 3Cu(NO3)2 + 4Ag

From the balanced equation, we can see that 3 moles of copper react with 8 moles of silver nitrate (AgNO3) to produce 4 moles of silver (Ag). Therefore, the ratio of moles of copper to moles of silver is 3:4.

Now, we can calculate the number of moles of silver deposited from 16.0g of copper.

1. Calculate the moles of copper:
Moles of copper = Mass of copper / molar mass of copper
Molar mass of copper (Cu) = 63.5 g/mol

Moles of copper = 16.0g / 63.5 g/mol = 0.252 mol

2. Calculate the moles of silver:
Moles of silver = (0.252 mol Cu) x (4 mol Ag / 3 mol Cu)
Moles of silver = 0.336 mol Ag

Therefore, 16.0g of copper will deposit 0.336 moles of silver from the silver trioxonitrate solution.