Question

what volume mL of 2.00M sulfuric acid is required to react completely with 0.3403 of copper (II) oxide

Answer 1

Solution:

Assuming the question asks to determine the following:

Q. What volume (mL) of 2.00 M sulfuric acid is required to react completely with 0.3403 moles of copper (II) oxide?

Answer:

Answer to the above question would be the following:

Step - 1:

The Balanced chemical equation would be the following:

   CuO + H₂SO₄  = CuSO₄ + H₂O ............................ (Equation - 1 )

Step - 2:

From above Equation - 1 we get, 1 mole H₂SO₄ reacts completely with 1 mole CuO ............

Step - 3:

From Equation - 1, we get to know, the following:

i.e. 0.3403 moles of H₂SO₄ will be required to react completely with 0.3403 moles of copper(II) oxide, i.e. CuO.....

   Moles of H₂SO₄ required = 0.3403 moles

Step - 4:

Let's assume Volume of H₂SO₄ required = V₁(mL)

Therefore, ...... since we know:

1 Liter = 1000 mL ....and 1.0 M = 1.0 mole/L = 1.0 mole / 1000 mL ....

We get the following.......

   (V₁ ) x ( 2.00 mole/ 1000 mL ) = 0.3403 moles of H₂SO₄

  V₁ = [ (0.3403 mole) x ( 1000 mL) ] / 2.00 mole

  V₁ = 170.15 mL

Therefore we get our Answer as below:

Volume of H₂SO₄ required (mL) = V₁ = 170.15 mL (Answer)