Calculate the moles of copper that will be displaced from a copper(2) tetraoxosulphate(5) by 6.5gram of zinc {cu=63.5, zinc =65}

To determine the moles of copper that can be displaced from copper(II) tetraoxosulphate(V) by 6.5 grams of zinc, we first need to understand the chemical reaction involved. Zinc can displace copper from copper(II) sulfate due to its higher reactivity. The balanced chemical equation for this reaction is:

Chemical Reaction

The reaction can be represented as:

Zn(s) + CuSO₄(aq) → ZnSO₄(aq) + Cu(s)

Step 1: Calculate Moles of Zinc

First, we need to find out how many moles of zinc we have in 6.5 grams. The molar mass of zinc (Zn) is 65 g/mol. We can use the formula:

Moles = Mass (g) / Molar Mass (g/mol)

Substituting the values:

Moles of Zn = 6.5 g / 65 g/mol = 0.1 moles

Step 2: Determine Moles of Copper Displaced

From the balanced equation, we see that 1 mole of zinc displaces 1 mole of copper. Therefore, if we have 0.1 moles of zinc, it will displace an equal amount of copper:

Moles of Cu displaced = Moles of Zn = 0.1 moles

Final Result

Thus, the moles of copper that will be displaced from copper(II) tetraoxosulphate(V) by 6.5 grams of zinc is 0.1 moles.

Summary

• Moles of zinc calculated: 0.1 moles
• Moles of copper displaced: 0.1 moles

This straightforward stoichiometric calculation illustrates how the reactivity of metals can be used to predict the outcome of a chemical reaction. If you have any further questions or need clarification on any part of this process, feel free to ask!