Question

Solid iron(iii) hydroxide decomposes to produce iron(iii) oxide and water vapor, according to the following reaction: 2fe(oh)3 → fe2o3 3h2o. if 0.75 l of water vapor is produced at stp,
a. how many grams of iron(iii) hydroxide were used?

Answer 1

The balanced chemical reaction is:

2Fe(OH)3 = Fe2O3 + 3H2O

We are given the amount of water vapor to be produced from the reaction. This will be the starting point of our calculations.

0.75 L H2O ( 1 mol / 22.4 L ) ( 2 mol Fe(OH)3 / 3 mol H2O ) ( 106.87 g / 1 mol ) = 2.39 g Fe(OH)3

Answer 2

2.39 g of iron(iii) hydroxide was used if 0.75 l of water vapor is produced at STP.

STP

STP is defined as standard temperature and pressure.

Volume at STP is 22.4 L.

The balanced chemical reaction is:

$2Fe(OH)_3 = Fe_2O_3 + 3H_2O$

Calculate grams of iron(iii) hydroxide as follows:-

$0.75 L H_2O ( 1 mol / 22.4 L ) ( 2 mol Fe(OH)_3 / 3 mol H_2O ) ( 106.87 g / 1 mol ) = 2.39 g Fe(OH)_3$

So, 2.39 g iron hydroxide was used.

Find more information about STP here,

https://brainly.com/question/26107741