Question

Смешали 100 г 100% гидроксида калия с 2г хоорила железа 3, найдите массу осадка образовавшегося в результате химической реакции? Срочно

Answer 1

Ответ на фотографии

Answer 2

Chemical Reaction Calculation

To find the mass of the precipitate formed as a result of the chemical reaction between 100 g of 100% potassium hydroxide and 2 g of iron(III) chloride, we can use the concept of limiting reagents and chemical equations.

The balanced chemical equation for the reaction between potassium hydroxide (KOH) and iron(III) chloride (FeCl3) is:

2KOH + FeCl3 → 2KCl + Fe(OH)3

Limiting Reagent Calculation

First, we need to determine the limiting reagent to find out how much of each reactant is consumed and which one limits the amount of product formed.

The molar mass of KOH is approximately 56.11 g/mol, and the molar mass of FeCl3 is approximately 162.2 g/mol.

- For KOH: 100 g / 56.11 g/mol = 1.78 moles - For FeCl3: 2 g / 162.2 g/mol = 0.0123 moles

Based on the balanced chemical equation, 2 moles of KOH react with 1 mole of FeCl3. Therefore, the molar ratio of KOH to FeCl3 is 2:1.

Since the moles of KOH are much higher than the moles of FeCl3, FeCl3 is the limiting reagent.

Calculation of Precipitate Mass

The limiting reagent (FeCl3) will completely react with the available KOH. From the balanced chemical equation, 1 mole of FeCl3 produces 1 mole of Fe(OH)3.

The molar mass of Fe(OH)3 is approximately 106.87 g/mol.

So, the mass of Fe(OH)3 formed can be calculated as follows:

0.0123 moles of FeCl3 * 106.87 g/mol = 1.31 grams of Fe(OH)3.

Therefore, the mass of the precipitate formed as a result of the chemical reaction is approximately 1.31 grams.