<u>Answer:</u> The volume of solution required is 0.0275 L.
<u>Explanation:</u>
To calculate the number of moles, we use the equation:
Given mass of copper = 4.24 g
Molar mass of copper = 63.55 g/mol
Putting values in above equation, we get:
![\text{Moles of copper}=\frac{4.24g}{63.55g/mol}=0.067mol](https://tex.z-dn.net/?f=%5Ctext%7BMoles%20of%20copper%7D%3D%5Cfrac%7B4.24g%7D%7B63.55g%2Fmol%7D%3D0.067mol)
The chemical equation for the reaction of potassium dichromate and copper follows:
![K_2Cr_2O_7+3Cu+7H_2SO_4\rightarrow 3CuSO_4+Cr_2(SO_4)_3+K_2SO_4+7H_2O](https://tex.z-dn.net/?f=K_2Cr_2O_7%2B3Cu%2B7H_2SO_4%5Crightarrow%203CuSO_4%2BCr_2%28SO_4%29_3%2BK_2SO_4%2B7H_2O)
By Stoichiometry of the reaction:
3 moles of copper reacts with 1 mole of potassium dichromate.
So, 0.067 moles of copper will react with =
of potassium dichromate
To calculate the volume of potassium dichromate, we use the equation:
![\text{Molarity of the solution}=\frac{\text{Moles of solute}}{\text{Volume of solution (in L)}}](https://tex.z-dn.net/?f=%5Ctext%7BMolarity%20of%20the%20solution%7D%3D%5Cfrac%7B%5Ctext%7BMoles%20of%20solute%7D%7D%7B%5Ctext%7BVolume%20of%20solution%20%28in%20L%29%7D%7D)
We are given:
Moles of potassium dichromate = 0.022 mol
Molarity of solution = 0.800 M
Putting values in above equation, we get:
![0.08mol/L=\frac{0.022mol}{\text{Volume of solution}}\\\\\text{Volume of solution}=0.0275L](https://tex.z-dn.net/?f=0.08mol%2FL%3D%5Cfrac%7B0.022mol%7D%7B%5Ctext%7BVolume%20of%20solution%7D%7D%5C%5C%5C%5C%5Ctext%7BVolume%20of%20solution%7D%3D0.0275L)
Hence, the volume of solution required is 0.0275 L.