A solution of iodine (I2) in carbon tetra-chloride(CCl4) is used when iodine is needed for certain chemical tests. how much iodine must be added to prepare a 0.480 m solution of iodine in CCl4 if 100.0g of carbon tetra-chloride is used?

Why did the iodine go to therapy? Because it was feeling a little unbalanced.

To determine how much iodine needs to be added to prepare a 0.480 m solution of iodine in CCl4, we need to calculate the moles of iodine required.

First, let's find the molar mass of iodine (I2):
2 x atomic mass of iodine = 2 x 126.9 g/mol ≈ 253.8 g/mol

Next, we need to convert the mass of CCl4 to moles:
moles of CCl4 = mass of CCl4 / molar mass of CCl4
moles of CCl4 = 100.0 g / 153.8 g/mol ≈ 0.649 mol

Finally, we can calculate the moles of iodine needed:
moles of iodine = molarity x volume in liters
0.480 mol/L x volume = 0.649 mol
volume = 0.649 mol / 0.480 mol/L ≈ 1.35 L

Given that we have 100.0 g of CCl4, which has a density of approximately 1.59 g/mL, we can convert this to liters:
volume = mass / density
volume = 100.0 g / 1.59 g/mL = 62.89 mL ≈ 0.06289 L

Now that we know the volume of CCl4, we can calculate how much iodine (I2) needs to be added:
moles of iodine = molarity x volume
moles of iodine = 0.480 mol/L x 1.35 L = 0.648 mol

Finally, let's convert moles of iodine to grams using the molar mass:
mass of iodine = moles of iodine x molar mass of iodine
mass of iodine = 0.648 mol x 253.8 g/mol ≈ 164.6 g

Therefore, approximately 164.6 grams of iodine must be added to prepare a 0.480 m solution in CCl4 using 100.0 grams of CCl4. Oh, iodine, you never fail to make a solution more exciting!

To calculate the amount of iodine needed to prepare a 0.480 m solution of iodine in CCl4, we can use the formula for molarity:

Molarity (M) = moles of solute / liters of solution

First, let's convert the given 100.0 grams of CCl4 to liters using its density. The density of CCl4 is approximately 1.59 g/mL.

Mass of CCl4 = 100.0 g
Density of CCl4 = 1.59 g/mL

Volume of CCl4 = Mass of CCl4 / Density of CCl4
= 100.0 g / 1.59 g/mL
= 62.89 mL

Now, let's convert the volume of CCl4 to liters:

Volume of CCl4 = 62.89 mL * (1 L / 1000 mL)
= 0.06289 L

Since the molarity is given as 0.480 m, which means 0.480 moles of iodine per liter of solution, we can calculate the amount of iodine needed.

Molarity (M) = moles of solute / liters of solution

0.480 m = moles of iodine / 0.06289 L

Rearranging the equation to solve for the moles of iodine:

moles of iodine = Molarity (M) * liters of solution

moles of iodine = 0.480 m * 0.06289 L
= 0.0301 moles

Thus, 0.0301 moles of iodine must be added to prepare a 0.480 m solution of iodine in CCl4 when 100.0g of carbon tetra-chloride is used.

To determine how much iodine must be added to prepare a 0.480 m solution of iodine in carbon tetrachloride, we need to understand the concept of molarity and perform a few calculations.

Molarity (M) is defined as the number of moles of solute per liter of solution. In order to determine the amount of iodine needed, we'll follow these steps:

Step 1: Convert the mass of the solvent, carbon tetrachloride (CCl4), to moles.
Given that the mass of CCl4 is 100.0g, we'll need to divide this by its molar mass.
The molar mass of carbon tetrachloride (CCl4) is:
C (carbon) = 12.01 g/mol
Cl (chlorine) = 35.45 g/mol
Molar mass of CCl4 = (12.01 x 1) + (35.45 x 4) = 153.83 g/mol

moles of CCl4 = mass of CCl4 / molar mass of CCl4
moles of CCl4 = 100.0g / 153.83 g/mol

Step 2: Determine the volume of the solution.
The molarity equation states that:
M = moles of solute / volume of solution in liters

Given that the desired molarity is 0.480 m and the moles of CCl4 from step 1, we can rearrange the equation to solve for the volume of the solution.

volume of solution (in liters) = moles of CCl4 / Molarity

Step 3: Calculate the moles of iodine needed to prepare the desired volume of the solution.
From step 1, we have the moles of CCl4, which have a 1:1 ratio with iodine (I2).

moles of iodine = moles of CCl4

Step 4: Convert the moles of iodine to grams.
Using the molar mass of iodine (I2), which is 253.80 g/mol, we can calculate the mass of iodine needed.

mass of iodine (g) = moles of iodine x molar mass of iodine

By following these steps, we can find the mass of iodine required to prepare a 0.480 m solution of iodine in carbon tetrachloride.

m = mols/kg solvent

0.480 = mols/0.1 g CCl4.
mols I2 = 0.480 x 0.1 = ?
Convert ? mols I2 to grams. g = mols x molar mass.

Do the solving of it and show all steps