What volume of 16M HNO3 is required to dissolve 0.50g of Cu metal in the following reaction?

Cu(s) + 4HNO3(aq) ---> Cu(NO3)2 + 2H2O + 2NO2

Dissolve? Or react...

how many moles of Cu? .5/atomicmassCu

how many moles of nitric acid? 4*molesCu

volume: molesNitriacid/16

Well, in order to find the volume of 16M HNO3 required to dissolve 0.50g of Cu metal, we need to do some calculations. But before we do, I just want to say that this reaction is pretty metal...literally!

Okay, let's get back to business. The first step is to figure out the number of moles of Cu using its molar mass. Since the molar mass of Cu is 63.55 g/mol, we can calculate that 0.50g of Cu is equal to 0.50/63.55 = 0.0079 moles.

According to the balanced equation, 4 moles of HNO3 react with 1 mole of Cu. Therefore, we need 4 times the number of moles of HNO3 to react completely with the given amount of Cu. So, we need 4 x 0.0079 = 0.0316 moles of HNO3.

Now, to find the volume of the 16M HNO3, we can use the formula:

Volume (in liters) = Moles / Molarity
= 0.0316 moles / 16 mol/L
= 0.00197875 L
≈ 1.98 mL

So, you would need approximately 1.98 mL of 16M HNO3 to dissolve 0.50g of Cu metal. And remember, if you need any more help, just call me...your friendly neighborhood Clown Bot!

To determine the volume of 16M HNO3 required to dissolve 0.50g of Cu metal, you need to calculate the mole ratio between Cu and HNO3, and then use it to convert the mass of Cu to moles. Finally, you can use the molarity and the obtained moles to find the volume of HNO3.

Step 1: Calculate the moles of Cu
The molar mass of Cu is 63.55 g/mol.
moles of Cu = mass / molar mass = 0.50g / 63.55 g/mol

Step 2: Determine the moles of HNO3
According to the balanced equation, the mole ratio between Cu and HNO3 is 1:4.
moles of HNO3 = 4 * moles of Cu

Step 3: Determine the volume of HNO3
Molarity (M) = moles / volume (L)
Rearrange the equation to solve for volume:
volume (L) = moles / Molarity

Let's substitute the values into the equation:
volume (L) = (4 * moles of Cu) / 16M

Now, let's calculate it.

moles of Cu = 0.50g / 63.55 g/mol
moles of HNO3 = 4 * (0.50g / 63.55 g/mol)
volume (L) = (4 * (0.50g / 63.55 g/mol)) / 16M

To determine the volume of 16M HNO3 required to dissolve 0.50g of Cu metal, we need to use stoichiometry.

Step 1: Start by balancing the equation:
Cu(s) + 4HNO3(aq) ---> Cu(NO3)2(aq) + 2H2O(l) + 2NO2(g)

Step 2: Calculate the molar mass of Cu(NO3)2:
Copper (Cu): 63.55 g/mol
Nitrogen (N): 14.01 g/mol
Oxygen (O): 16.00 g/mol
Molar mass of Cu(NO3)2 = (63.55g/mol) + 2 * [(14.01g/mol) + 3 * (16.00g/mol)] = 187.55 g/mol

Step 3: Convert the given mass of Cu metal to moles:
Given mass = 0.50g
Molar mass of Cu = 63.55 g/mol
Number of moles = 0.50g / 63.55 g/mol = 0.00787 mol

Step 4: Use stoichiometry to determine the ratio between HNO3 and Cu(NO3)2.
From the balanced equation, we see that it takes 4 moles of HNO3 to react with 1 mole of Cu. Therefore, the ratio is 4:1.

Step 5: Calculate the moles of HNO3 needed:
Moles of HNO3 = (moles of Cu) * (4 moles of HNO3 / 1 mole of Cu) = 0.00787 mol * (4 mol/1 mol) = 0.0315 mol

Step 6: Calculate the volume of 16M HNO3 needed:
Molarity (M) = Moles / Volume (L)
Volume (L) = Moles / Molarity

Given Molarity of HNO3 = 16 M
Moles of HNO3 = 0.0315 mol

Volume = 0.0315 mol / 16 M = 0.00196875 L = 1.97 mL

Therefore, approximately 1.97 mL of 16M HNO3 is required to dissolve 0.50g of Cu metal in the reaction.