what mass of copper II nitrate would be produced from the complete reaction of 45.6g of copper according to the chemical reaction :
Cu + 2 AgNO3 (can't make it a small 3, sorry)----Cu(NO3) + 2 Ag
To determine the mass of copper(II) nitrate produced, we first need to balance the chemical equation:
Cu + 2 AgNO3 → Cu(NO3)2 + 2 Ag
From the balanced equation, we can see that one mole of copper reacts with two moles of silver nitrate to produce one mole of copper(II) nitrate.
To calculate the mass of copper(II) nitrate, we need to follow these steps:
Step 1: Convert the mass of copper (Cu) to moles.
Step 2: Use the mole ratio from the balanced equation to determine the number of moles of copper(II) nitrate produced.
Step 3: Convert the moles of copper(II) nitrate to mass.
Let's go step by step:
Step 1: Convert the mass of copper to moles.
The molar mass of copper (Cu) is 63.55 g/mol.
Mass of copper (Cu) = 45.6 g
Number of moles = Mass / Molar mass
Number of moles of copper = 45.6 g / 63.55 g/mol ≈ 0.718 moles
Step 2: Use the mole ratio to determine the moles of copper(II) nitrate.
From the balanced equation, we see that the mole ratio between copper(Cu) and copper(II) nitrate (Cu(NO3)2) is 1:1.
Therefore, 0.718 moles of copper will produce 0.718 moles of copper(II) nitrate.
Step 3: Convert moles of copper(II) nitrate to mass.
The molar mass of copper(II) nitrate (Cu(NO3)2) is 187.56 g/mol.
Mass of copper(II) nitrate = Moles × Molar mass
Mass of copper(II) nitrate = 0.718 moles × 187.56 g/mol ≈ 134.95 g
Therefore, approximately 134.95 grams of copper(II) nitrate would be produced from the complete reaction of 45.6 grams of copper.
To determine the mass of copper(II) nitrate produced, we need to use stoichiometry.
First, we need to balance the chemical equation:
Cu + 2 AgNO3 → Cu(NO3)2 + 2 Ag
Now, let's find the molar mass of copper(II) nitrate (Cu(NO3)2).
Cu: 1 atom of copper has a molar mass of 63.55 g/mol.
N: 2 atoms of nitrogen have a molar mass of 14.01 g/mol each, so the total is 28.02 g/mol.
O: 6 atoms of oxygen have a molar mass of 16.00 g/mol each, so the total is 96.00 g/mol.
Adding the masses together:
63.55 g/mol (Cu) + 28.02 g/mol (N) + 96.00 g/mol (O) + 96.00 g/mol (O) = 283.57 g/mol (Cu(NO3)2)
Now we can calculate the number of moles of copper used. To do this, we divide the mass of copper by its molar mass:
45.6 g (Cu) / 63.55 g/mol (Cu) = 0.7179 mol Cu
According to the balanced equation, the ratio of copper to copper(II) nitrate is 1:1, meaning that for every mole of copper consumed, we will produce 1 mole of copper(II) nitrate.
Therefore, the number of moles of copper(II) nitrate produced is also 0.7179 mol Cu(NO3)2.
To calculate the mass of copper(II) nitrate, we multiply the number of moles by its molar mass:
0.7179 mol (Cu(NO3)2) * 283.57 g/mol (Cu(NO3)2) = 203.84 g Cu(NO3)2
Therefore, the mass of copper(II) nitrate produced from the reaction of 45.6 g of copper is 203.84 grams.
The equation is
Cu + 2AgNO3 ==> Cu(NO3)2 + 2Ag
See the solved example below. Just follow the steps.
http://www.jiskha.com/science/chemistry/stoichiometry.html