If 4.56 mol of zinc react with excess copper (ii) sulphate, how many moles of precipitate will be formed?

Zn + CuSO4 = Cu + ZnSO4

same number of moles of each

To determine the number of moles of the precipitate formed, we need to first identify the balanced chemical equation for the reaction between zinc and copper (II) sulfate. The equation is as follows:

Zn(s) + CuSO4(aq) -> ZnSO4(aq) + Cu(s)

According to the balanced equation, one mole of zinc reacts with one mole of copper (II) sulfate to produce one mole of zinc sulfate and one mole of copper.

Since we have 4.56 moles of zinc, we can conclude that 4.56 moles of copper (II) sulfate will react.

Therefore, the number of moles of precipitate formed would also be 4.56 moles.

To find out how many moles of precipitate will be formed, we need to use the balanced chemical equation for the reaction between zinc and copper (II) sulfate.

The balanced equation is:
Zn + CuSO4 → ZnSO4 + Cu

From the equation, we can see that 1 mole of zinc reacts with 1 mole of copper (II) sulfate to produce 1 mole of zinc sulfate and 1 mole of copper.

Since we are given that 4.56 mol of zinc is reacting, we can assume that the reaction will proceed until all the zinc is consumed.

Therefore, the number of moles of precipitate formed will be equal to the number of moles of copper produced. According to the balanced equation, this will be 1 mole of copper.

So, 4.56 moles of zinc will react to produce 1 mole of precipitate (copper).

Thus, 4.56 moles of precipitate will be formed.