Aluminum reacts with excess copper(II) sulfate according to the unbalanced reaction Al(s) + CuSO4(aq) −→
Al2(SO4)3(aq) + Cu(s)
If 2.98 g of Al react and the percent yield of
Cu is 46.4%, what mass of Cu is produced?
Answer in units of g.

The mass of Cu produced is 4.88 g

Explanation:

The number of moles is defined as the ratio of the mass of a substance to its molar mass.

The equation used is:

......(1)

Given mass of aluminum = 2.98 g

Molar mass of aluminum = 27 g/mol

Plugging values in equation 1:

The given chemical equation follows:

By the stoichiometry of the reaction:

If 2 moles of aluminum produces 3 moles of Cu

So, 0.1104 moles aluminium will produce = of Cu

Molar mass of Cu = 63.5 g/mol

Plugging values in equation 1:

The percent yield of a reaction is calculated by using an equation:

......(2)

Given values:

% yield of product = 46.4 %

Theoretical value of the product = 10.516 g

Plugging values in equation 2, we get:

Hence, the mass of Cu produced is 4.88 g

i think that the answer is c