Question

When 0.5 g of powdered iron (III) oxide was added to 100 cm3 of hydrogen peroxide, water and oxygen were produced. Iron (III) oxide was not used up in the reaction. Based on the information, which of the following is likely to increase the rate formation of the products? Replacing the powdered iron oxide with its cubical crystals Using 150 cm3 of hydrogen peroxide Removing iron oxide from the reaction mixture Using 1.0 gram of iron oxide

Answer 1

Answer:

Using 1.0 gram of iron oxide.

Explanation:

• Rate of the reaction depends on many factors:

The concentration of the reactants.

The surface area of the reactants or catalyst.

The amount of the catalyst.

Hydrogen peroxide is the reactant and iron (III) oxide is the catalyst.

• If we display the various choices:

Replacing the powdered iron oxide with its cubical crystals:

This will decrease the surface area of the catalyst exposed to the solution, so the rate formation of the products will decrease.

Using 150 cm³ of hydrogen peroxide:

The volume of the reactant does not affect the concentration of the reactants, so changing the volume has no effect on the rate formation of the products.

Removing iron oxide from the reaction mixture:

Removing the catalyst will decrease (may stop) the rate formation of the products.

Using 1.0 gram of iron oxide:

This will increase the amount of the catalyst used, and so it will increase the rate formation of the products.

So, the right choice is:

the rate formation of the products