Question

At very high temperatures, copper(II) sulfate undergoes the reaction CuSO4(s) --> CuO (s) + SO3 (g)

What kind of reaction is this?

If 319.22 g CuSO4(s) reacted completely in the reaction, how many grams of CuO(s) would be produced?

Answer 1

Answer: a) Decomposition

b) 159.0 g of CuO(s) would be produced.

Explanation:

Decomposition reaction is a chemical reaction in which one reactant gives two or more than two products. They are endothermic reactions as energy is required to break the bonds of the reactants.

`CuSO_4(s)\rightarrow CuO(s)+SO_3(g)`

As can be seen from the given balanced reaction:

1 mole of
`CuSO_4` gives 1 mole of
`CuO`.

Thus 159.6 g of
`CuSO_4` gives 79.5 g of
`CuO`.

319.22 g of
`CuSO_4` will give=
`(79.5)/(159.6)* 319.22=159.0g`of
`CuO`.

Answer 2

Answer : This is a type of decomposition reaction. The mass of copper oxide produced would be, 159 grams

Solution : Given,

Mass of copper sulfate = 319.22 g

Molar mass of copper sulfate = 159.6 g/mole

Molar mass of copper oxide = 79.5 g/mole

First we have to calculate the moles of copper sulfate.

`\text{Moles of }CuSO_4=\frac{\text{Mass of }CuSO_4}{\text{Molar mass of }CuSO_4}=(319.22g)/(159.6g/mole)=2moles`

Now we have to calculate the moles of copper oxide.

The balanced chemical reaction is,

`CuSO_4(s)\rightarrow CuO(s)+SO_3(g)`

This reaction is a decomposition reaction in which the larger reactant molecule decomposes to give two or more new products.

From the reaction, we conclude that

As, 1 mole of copper sulfate decomposes to produce 1 mole of copper oxide

So, 2 moles of copper sulfate decomposes to produce 2 moles of copper oxide

Now we have to calculate the mass of copper oxide.

`\text{Mass of }CuO=\text{Moles of }CuO* \text{Molar mass of }CuO`

`\text{Mass of }CuO=(2mole)* (79.5g/mole)=159g`

Therefore, the mass of copper oxide produced would be, 159 grams