Question

Molarity, abbreviated M, is defined as the concentration of a solution expressed as moles of solute per liter of
solution. How many milliliters of 4.00 M H2SO4 are required to react with 1.60 g of Cuo according to CuO(s) + H2SO4(aq)-->CuSO4(aq)+H2O(l)​

Answer 1

Answer:

5 mL H₂SO₄

Explanation:

The equation for the reaction is;

CuO(s) + H₂SO₄(aq)→ CuSO₄(aq)+H₂O(l)

We are given;

Molarity of H₂SO₄ = 4.00 M

Mass of CuO = 1.6 g

We are required to calculate the volume of H₂SO₄

First; we need to determine the number of moles of CuO

Moles = Mass ÷ Molar mass

Molar mass of CuO =79.545 g/mol

Mass of Cu =1.6 g

Moles of CuO = 1.6 g ÷ 79.545 g/mol

                       = 0.020 moles

Second; we determine the number of moles of H₂SO₄ that reacted with CuO.

From the equation 1 mole of CuO reacts with 1 mole of H₂SO₄

Therefore;

0.020 moles of CuO will react with 0.020 moles H₂SO4

Third; we calculate the volume of H₂SO₄

Molarity is given by dividing the number of moles by volume.

Thus;

Volume = Moles ÷ Molarity

In this case;

Volume = 0.020 moles ÷ 4.00 M

             = 0.005 L

But; 1 L = 1000 mL

Therefore; Volume = 5 mL

Hence the volume of H₂SO₄ required to react with CuO is 5 mL