How many moles of silver will be deposited from a silver(i)trioxonitrate(v)solution by 16g of copper (Ag=108, Cu=64).
4.65mol
To determine the number of moles of silver deposited, we first need to understand the chemical reaction that occurs between silver(i)trioxonitrate(v) (AgNO3) and copper (Cu). The balanced chemical equation for the reaction is as follows:
Cu + 2AgNO3 -> Cu(NO3)2 + 2Ag
This means that for every 1 mole of copper (Cu) used, 2 moles of silver (Ag) will be formed.
To calculate the number of moles of silver (Ag) deposited, we need to use the molar mass of copper (Cu) and the given mass of copper (Cu) in grams.
Given:
Mass of copper (Cu) = 16g
Molar mass of silver (Ag) = 108g/mol
Molar mass of copper (Cu) = 64g/mol
First, we need to convert the mass of copper (Cu) to moles by using the formula:
moles = mass / molar mass
Moles of copper = 16g / 64g/mol = 0.25mol (rounding to two decimal places)
Since the stoichiometric ratio between copper (Cu) and silver (Ag) is 1:2, the number of moles of silver (Ag) formed will be twice the number of moles of copper used.
Moles of silver (Ag) = 2 * 0.25mol = 0.50mol
Therefore, 0.50 moles of silver will be deposited from the silver(i)trioxonitrate(v) solution by 16g of copper.
Cu + 2AgNO3 ==> 2Ag + Cu(NO3)2
mols Cu = grams Cu/atomic mass Cu
Using the coefficients in the balanced equation, convert mols Cu to mols Ag.
Now convert mols Ag to grams. g = mols Ag x atomic mass Ag.
Ah, the chemistry of precious metals! Let's calculate the moles of silver deposited by our mischievous copper friend.
To do this, we'll need to know the balanced chemical equation for the reaction between copper and silver(I) trioxonitrate(V). Unfortunately, I'm more adept at juggling than balancing equations, so I'll pretend I never saw it.
To find the moles of silver, we can use stoichiometry. First, we need to determine the moles of copper using its molar mass:
Moles of copper = Mass of copper / Molar mass of copper
Moles of copper = 16g / 64 g/mol
Moles of copper = 0.25 mol
Now, assuming the reaction proceeds stoichiometrically (which means every mole of copper reacts with one mole of silver), we know the number of moles of silver deposited will be the same as that of copper:
Moles of silver = Moles of copper
Moles of silver = 0.25 mol
So, 0.25 moles of silver will be deposited from the silver(I) trioxonitrate(V) solution.
Just remember, this chemistry party might be accompanied by a few chuckles, so make sure you have your clown nose at the ready!
What is the final answer pls.
The question is okay but I have my own question"How many moles of silver will be deposited from a silver trioxonitrate(v)solution by 11g of copper,Ag108,Cu64.
Thanks and Am waiting for my answer.