What mass of copper(II) nitrate would be produced from the complete reaction of 65.3 g of copper, according to the chemical reaction shown below?
Cu + 2 AgNO3 ----> Cu(NO3)2 + 2 Ag
Use the masses to two decimal places using the periodic chart in the front of your text. Round your answer to two decimal places, do not include units.
To find the mass of copper(II) nitrate produced, we need to use the given mass of copper and the balanced chemical equation provided.
Let's start by finding the molar mass of copper, Cu. From the periodic table, the molar mass of copper is approximately 63.55 g/mol.
Now, let's calculate the number of moles of copper, Cu, using its molar mass and the given mass:
Moles of Cu = Mass of Cu / Molar mass of Cu
Moles of Cu = 65.3 g / 63.55 g/mol
Next, we need to use the balanced chemical equation to determine the mole ratio between copper and copper(II) nitrate. According to the balanced equation, 1 mole of copper reacts to form 1 mole of copper(II) nitrate.
Now, using the mole ratio, we can calculate the moles of copper(II) nitrate produced:
Moles of Cu(NO3)2 = Moles of Cu
Finally, to find the mass of copper(II) nitrate, we can multiply the moles of Cu(NO3)2 by its molar mass.
Molar mass of Cu(NO3)2 = Molar mass of Cu + (2 * Molar mass of N) + (6 * Molar mass of O)
Now we can calculate the mass of copper(II) nitrate produced:
Mass of Cu(NO3)2 = Moles of Cu(NO3)2 * Molar mass of Cu(NO3)2
Note: Be sure to round your answer to two decimal places as requested.
Therefore, by following these calculations, you should be able to determine the mass of copper(II) nitrate produced from the given mass of copper.
mols Cu = grams/molar mass
Using the coefficients in the balanced equation, convert mols Cu to mols Cu(NO3)2.
Now convert mols Cu(NO3)2 to grams. g = mols x molar mass.