What mass of copper(II) nitrate would be produced from the complete reaction of 45.6 g of copper, according to the chemical reaction shown below?

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

convert to moles.

Each mole of Cu will produce 1 mole of Cu(NO3)2
convert to grams

is the answer 135 g?

Well, let's do some math, shall we? According to the balanced chemical equation, we see that 1 mole of copper reacts with 2 moles of AgNO3 to produce 1 mole of Cu(NO3)2. Now, the molar mass of copper is about 63.55 g/mol. So, to find the moles of copper, we divide the mass (45.6g) by the molar mass of copper to get 0.716 moles of copper. Since the mole ratio between copper and copper(II) nitrate is 1:1, we can now confidently say that 0.716 moles of copper(II) nitrate will be produced. To find the mass, we multiply the number of moles by the molar mass of copper(II) nitrate (187.55 g/mol), which gives us approximately 134.22 g of copper(II) nitrate. Voila!

To find the mass of copper(II) nitrate produced, we need to first determine the balanced chemical equation. From the given chemical reaction:

Cu + 2 AgNO3 → Cu(NO3)2 + 2 Ag

The stoichiometry of the reaction shows that 1 mole of copper (Cu) reacts with 2 moles of silver nitrate (AgNO3) to produce 1 mole of copper(II) nitrate (Cu(NO3)2) and 2 moles of silver (Ag).

To find the mass of copper(II) nitrate produced, we will follow these steps:

Step 1: Calculate the molar mass of copper (Cu).
The molar mass of copper (Cu) is 63.55 g/mol.

Step 2: Convert the mass of copper (Cu) given to moles.
The number of moles of copper (Cu) can be calculated using the formula:

moles = mass / molar mass

moles of Cu = 45.6 g / 63.55 g/mol
moles of Cu ≈ 0.72 mol

Step 3: Use the balanced equation to determine the mole ratio between copper (Cu) and copper(II) nitrate (Cu(NO3)2).
From the balanced equation, we know that 1 mole of copper (Cu) reacts to form 1 mole of copper(II) nitrate (Cu(NO3)2).

Step 4: Convert the moles of copper(II) nitrate (Cu(NO3)2) to mass using its molar mass.
The molar mass of copper(II) nitrate (Cu(NO3)2) is:
63.55 g/mol (molar mass of Cu) + (2 x (14.01 g/mol) (molar mass of N) + 6 x 16.00 g/mol) (molar mass of O)
= 63.55 g/mol + 28.02 g/mol + 96.00 g/mol
= 187.57 g/mol

mass of Cu(NO3)2 = moles of Cu(NO3)2 x molar mass of Cu(NO3)2
mass of Cu(NO3)2 = 0.72 mol x 187.57 g/mol
mass of Cu(NO3)2 ≈ 135.18 g

Therefore, approximately 135.18 grams of copper(II) nitrate would be produced from the complete reaction of 45.6 grams of copper.

To find the mass of copper(II) nitrate produced, we need to use the balanced chemical equation and the molar mass of copper(II) nitrate.

First, let's calculate the molar mass of copper(II) nitrate (Cu(NO3)2):
Cu: 1 atom × 63.55 g/mol = 63.55 g/mol
N: 2 atoms × 14.01 g/mol = 28.02 g/mol
O: 6 atoms × 16.00 g/mol = 96.00 g/mol

Adding these values together, we get:
63.55 g/mol + 28.02 g/mol + 96.00 g/mol = 187.57 g/mol

Next, we need to determine the molar ratio between copper and copper(II) nitrate by looking at the balanced chemical equation:
Cu + 2 AgNO3 → Cu(NO3)2 + 2 Ag

According to the equation, the ratio between copper and copper(II) nitrate is 1:1. This means that 1 mole of copper will produce 1 mole of copper(II) nitrate.

Now, let's calculate the number of moles of copper using its molar mass:
Molar mass of copper = 63.55 g/mol
Moles of copper = mass / molar mass
Moles of copper = 45.6 g / 63.55 g/mol ≈ 0.717 mol

Since the molar ratio between copper and copper(II) nitrate is 1:1, the number of moles of copper(II) nitrate produced is also 0.717 mol.

Finally, we can determine the mass of copper(II) nitrate produced by multiplying the number of moles by its molar mass:
Mass of copper(II) nitrate = moles × molar mass
Mass of copper(II) nitrate = 0.717 mol × 187.57 g/mol ≈ 134.61 g

Therefore, approximately 134.61 grams of copper(II) nitrate would be produced from the complete reaction of 45.6 grams of copper.