23 Дар натиҷаи ҳал кардани 270 г нуқра дар кислотаи сулфати консентронида чанд литр (ш. м.) газ ҳосил мешавад?

Solution:

The reaction between silver (Ag) and concentrated sulfuric acid (H₂SO₄) produces silver sulfate (Ag₂SO₄), sulfur dioxide (SO₂), and water (H₂O).

The balanced chemical equation is:

\[ 2\text{Ag} + 2\text{H}_2\text{SO}_4 \text{(conc.)} \rightarrow \text{Ag}_2\text{SO}_4 + \text{SO}_2 + 2\text{H}_2\text{O} \]

We are given 270 g of silver (Ag). We need to find the volume of sulfur dioxide (SO₂) gas produced at standard conditions (STP).

First, calculate the molar mass of silver (Ag).

Molar mass of Ag = 107.87 g/mol.

Now, calculate the number of moles of silver in 270 g:

\[ n(\text{Ag}) = \frac{\text{mass}}{\text{molar mass}} = \frac{270 \text{ g}}{107.87 \text{ g/mol}} \approx 2.503 \text{ mol} \]

From the balanced chemical equation, 2 moles of Ag produce 1 mole of SO₂. So, the mole ratio of Ag to SO₂ is 2:1.

Calculate the moles of SO₂ produced:

\[ n(\text{SO}_2) = n(\text{Ag}) \times \frac{1 \text{ mol SO}_2}{2 \text{ mol Ag}} = 2.503 \text{ mol Ag} \times \frac{1}{2} \approx 1.2515 \text{ mol} \]

At standard temperature and pressure (STP), 1 mole of any gas occupies 22.4 liters.

Now, calculate the volume of SO₂ gas produced:

\[ \text{Volume of SO}_2 = n(\text{SO}_2) \times 22.4 \text{ L/mol} \]

\[ \text{Volume of SO}_2 = 1.2515 \text{ mol} \times 22.4 \text{ L/mol} \approx 28.03 \text{ L} \]

Rounding to an appropriate number of significant figures (based on 270 g, which has 3 significant figures):

\[ \text{Volume of SO}_2 \approx 28.0 \text{ L} \]

Answer: 28.0 литр