If 0.188 moles of zinc reacts with excess lead(IV) sulfate, how many grams of zinc sulfate would be produced in the following reaction?

To determine the grams of zinc sulfate produced, we need to first write the balanced equation for the reaction between zinc and lead(IV) sulfate.

The reaction can be represented as follows:
Zn + Pb(SO4)2 → ZnSO4 + Pb

From the balanced equation, we can see that one mole of zinc reacts with one mole of lead(IV) sulfate to produce one mole of zinc sulfate.

The molar mass of zinc sulfate (ZnSO4) is 161.4 g/mol.

To calculate the grams of zinc sulfate produced, we can use the mole-to-gram conversion. By multiplying the number of moles of zinc sulfate by its molar mass, we can determine the grams produced.

Given that 0.188 moles of zinc reacts, we can conclude that:

0.188 moles of zinc × (161.4 g/mol of zinc sulfate) = 30.4 grams of zinc sulfate

Therefore, 0.188 moles of zinc reacting with excess lead(IV) sulfate would produce approximately 30.4 grams of zinc sulfate.

To determine the grams of zinc sulfate produced in the reaction, you'll need to use stoichiometry, which relates the amount of one substance in a chemical reaction to the amount of another substance in the same reaction.

First, let's balance the equation for the reaction between zinc and lead(IV) sulfate:

Zn + Pb(SO4)2 → ZnSO4 + Pb

The balanced equation shows that 1 mole of zinc reacts with 1 mole of lead(IV) sulfate to produce 1 mole of zinc sulfate.

Given that 0.188 moles of zinc reacts, we can determine the number of moles of zinc sulfate produced:

0.188 moles Zn × (1 mole ZnSO4 / 1 mole Zn) = 0.188 moles ZnSO4

Now, we can calculate the mass of zinc sulfate produced using its molar mass. The molar mass of zinc sulfate (ZnSO4) is approximately:

Zn: 65.38 g/mol
S: 32.07 g/mol
O: 16.00 g/mol (4 atoms)
Total: 161.38 g/mol

Mass of zinc sulfate = 0.188 moles ZnSO4 × 161.38 g/mol = 30.38 grams

Therefore, if 0.188 moles of zinc reacts with excess lead(IV) sulfate, approximately 30.38 grams of zinc sulfate would be produced in this reaction.