What mass of Cu is in 300.0 mL of .200 M Cu2SO3?My work is attached but I'm not sure if this is the right approach. I found the molar mass of the compound, the moles of the compound, and the total mass for the compound.Then I tried to find a mole ratio between copper and the compound by dividing the molar mass for Cu2 by the compound molar mass, coming up with a factor of .6136. I took this factor and multiplied it by the total mass of the compound. I got 7.627 g of Cu2.Could you explain the steps to isolate the copper mass in this compound? ### Calculation of Molar Mass and Mass Conversions for Cu\(_2\)SO\(_3\)**1. Calculate the Molar Mass of Cu\(_2\)SO\(_3\):**- The formula for the molar mass of Cu\(_2\)SO\(_3\) is: \[ (2 \times 63.546) + (32.06) + (3 \times 15.999) \]- Calculation: \[ = 207.149 \, \text{g/mol} \, \text{Cu\(_2\)SO\(_3\)} \]**2. Determine the Moles of Cu\(_2\)SO\(_3\):**- Given: \[ \text{Volume} = 300.0 \, \text{mL} \times 10^{-3} \, \text{L/mL} = 0.300 \, \text{L} \] \[ \text{Concentration} = 0.200 \, \text{M} \]- Calculation of moles: \[ 0.300 \, \text{L} \times 0.200 \, \text{M} = 0.06 \, \text{mol Cu\(_2\)SO\(_3\)} \]**3. Calculate the Mass of Cu\(_2\)SO\(_3\):**- Formula: \[ \text{mass} = \text{moles} \times \text{molar mass} \]- Calculation: \[ 0.06 \, \text{mol} \times \frac{207.149 \, \text{g}}{\text{mol}} = 12.43 \, \text{g Cu\(_2\)SO\(_3\)} \]**4. Calculate Molar Mass of Cu\(_2\):**- Formula: \[ \text{molar mass of Cu\(_2\)} = (2 \times 63.546) \]- Calculation: \[ = 127.092 \, \text{g/mol} \, \text{Cu\(_2\)} \]**

Given that, the volume of Cu2SO3 is V = 300 mL = 0.3 L,The concentration is C = 0.200 M.We have to…

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What mass of Cu is in 300.0 mL of .200 M Cu₂SO₃?

My work is attached but I'm not sure if this is the right approach. I found the molar mass of the compound, the moles of the compound, and the total mass for the compound.

Then I tried to find a mole ratio between copper and the compound by dividing the molar mass for Cu₂ by the compound molar mass, coming up with a factor of .6136. I took this factor and multiplied it by the total mass of the compound. I got 7.627 g of Cu₂.

Could you explain the steps to isolate the copper mass in this compound?

### Calculation of Molar Mass and Mass Conversions for Cu\(_2\)SO\(_3\)

**1. Calculate the Molar Mass of Cu\(_2\)SO\(_3\):**

- The formula for the molar mass of Cu\(_2\)SO\(_3\) is:
\[
(2 \times 63.546) + (32.06) + (3 \times 15.999)
\]
- Calculation:
\[
= 207.149 \, \text{g/mol} \, \text{Cu\(_2\)SO\(_3\)}
\]

**2. Determine the Moles of Cu\(_2\)SO\(_3\):**

- Given:
\[
\text{Volume} = 300.0 \, \text{mL} \times 10^{-3} \, \text{L/mL} = 0.300 \, \text{L}
\]
\[
\text{Concentration} = 0.200 \, \text{M}
\]
- Calculation of moles:
\[
0.300 \, \text{L} \times 0.200 \, \text{M} = 0.06 \, \text{mol Cu\(_2\)SO\(_3\)}
\]

**3. Calculate the Mass of Cu\(_2\)SO\(_3\):**

- Formula:
\[
\text{mass} = \text{moles} \times \text{molar mass}
\]
- Calculation:
\[
0.06 \, \text{mol} \times \frac{207.149 \, \text{g}}{\text{mol}} = 12.43 \, \text{g Cu\(_2\)SO\(_3\)}
\]

**4. Calculate Molar Mass of Cu\(_2\):**

- Formula:
\[
\text{molar mass of Cu\(_2\)} = (2 \times 63.546)
\]
- Calculation:
\[
= 127.092 \, \text{g/mol} \, \text{Cu\(_2\)}
\]

**

Expert Solution

Step 1: Data and formula

Given that, the volume of Cu₂SO₃ is V = 300 mL = 0.3 L,

The concentration is C = 0.200 M.

We have to calculate the mass of Cu present in that solution.

Formula:

Number of moles = concentration × volume.
Molality is the number of moles of solute present per litre of solution.

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