When copper (II) nitrate reacts with sodium hydroxide, copper (II) hydroxide is produced. How many grams of copper (II) hydroxide can be prepared from 2.7 grams of copper (II) nitrate reacting with sodium hydroxide?
Cu(NO3)2 + 2NaOH ==> Cu(OH)2 + 2NaNO3
Moles Cu(NO3)2 = grams/molar mass = ?
Look at the coefficients in the balanced equation and see 1 mol Cu(OH)2 producerd from 1 mol Cu(NO3)2 used.
Then grams Cu(OH)2 = mols x molar mass = ?
Post your work if you get stuck.
Well, well, well, it seems we have a chemical reaction on our hands! Let's find out how much copper (II) hydroxide we can produce, shall we?
First, let's write out the balanced equation:
Cu(NO3)2 + 2 NaOH → Cu(OH)2 + 2 NaNO3
According to the equation, the molar ratio between Cu(NO3)2 and Cu(OH)2 is 1:1. So, we need to find the molar mass of Cu(OH)2 to calculate the grams of it.
Cu(OH)2 has a molar mass of approximately 97.56 g/mol.
Now, let's calculate the moles of Cu(NO3)2 using its molar mass:
2.7 g Cu(NO3)2 * (1 mol Cu(NO3)2 / molar mass of Cu(NO3)2) = X moles Cu(NO3)2
Next, using the 1:1 molar ratio, we can say that the moles of Cu(OH)2 produced will also be X.
Finally, we can calculate the grams of Cu(OH)2:
X moles Cu(OH)2 * (molar mass of Cu(OH)2 / 1 mol Cu(OH)2) = Y grams Cu(OH)2
And there you have it! The grams of copper (II) hydroxide that can be prepared from 2.7 grams of copper (II) nitrate reacting with sodium hydroxide.
To determine the number of grams of copper (II) hydroxide that can be prepared from 2.7 grams of copper (II) nitrate, we need to consider the stoichiometry of the reaction. The balanced equation for the reaction is as follows:
Cu(NO3)2 + 2NaOH -> Cu(OH)2 + 2NaNO3
From the equation, we can see that 1 mole of copper (II) nitrate reacts with 2 moles of sodium hydroxide to produce 1 mole of copper (II) hydroxide.
1 mole of copper (II) nitrate has a molar mass of 187.56 g/mol, while 1 mole of copper (II) hydroxide has a molar mass of 97.56 g/mol.
Therefore, we can calculate the number of moles of copper (II) hydroxide produced from 2.7 grams of copper (II) nitrate as follows:
2.7 g Cu(NO3)2 * (1 mol Cu(NO3)2 / 187.56 g Cu(NO3)2) * (1 mol Cu(OH)2 / 1 mol Cu(NO3)2) * (97.56 g Cu(OH)2 / 1 mol Cu(OH)2) = X grams of Cu(OH)2
Calculating this expression will give us the number of grams of copper (II) hydroxide that can be prepared from 2.7 grams of copper (II) nitrate.
To determine the grams of copper (II) hydroxide produced, we need to first write a balanced equation for the reaction between copper (II) nitrate and sodium hydroxide:
Cu(NO3)2 + 2NaOH → Cu(OH)2 + 2NaNO3
From the balanced equation, we can see that the ratio of copper (II) nitrate to copper (II) hydroxide is 1:1. This means that for every 1 mole of copper (II) nitrate, we will obtain 1 mole of copper (II) hydroxide.
To calculate the moles of copper (II) hydroxide produced, we need to convert the given mass of copper (II) nitrate to moles. We will use the molar mass of copper (II) nitrate to perform this conversion.
The molar mass of copper (II) nitrate (Cu(NO3)2) can be calculated as follows:
Cu: 63.55 g/mol
N: 14.01 g/mol
O: 16.00 g/mol (3 oxygen atoms)
Molar mass of Cu(NO3)2 = (63.55 g/mol) + (2 * (14.01 g/mol)) + (6 * (16.00 g/mol)) = 187.55 g/mol
Now, we can calculate the moles of copper (II) nitrate:
moles = mass / molar mass = 2.7 g / 187.55 g/mol ≈ 0.0144 mol
Since the ratio of copper (II) nitrate to copper (II) hydroxide is 1:1, the moles of copper (II) hydroxide produced will also be 0.0144 mol.
Finally, we can calculate the mass of copper (II) hydroxide using its molar mass.
The molar mass of copper (II) hydroxide (Cu(OH)2) can be calculated as follows:
Cu: 63.55 g/mol
O: 16.00 g/mol (2 oxygen atoms)
H: 1.01 g/mol (2 hydrogen atoms)
Molar mass of Cu(OH)2 = (63.55 g/mol) + (2 * (1.01 g/mol)) + (2 * (16.00 g/mol)) = 97.55 g/mol
Now, we can calculate the mass of copper (II) hydroxide:
mass = moles * molar mass = 0.0144 mol * 97.55 g/mol ≈ 1.41 g (rounded to two decimal places)
Therefore, approximately 1.41 grams of copper (II) hydroxide can be prepared from 2.7 grams of copper (II) nitrate reacting with sodium hydroxide.