Question

Вычислить массу сероводорода, который выделяется при взаимодействии 108 г алюминия с концентрированной серной кислотой при нагревании, если выход продуктов реакции 75%.

Answer 1

1.     Записываем ур-ие реакции:

8Al + 15H2SO4 = 4Al2(SO4)3 + 3H2S + 12H2O

2.     Вычисляем молярные массы реагирующих в-в

Алюминий  (Al ) - 27 г/моль

Сероводород (H2S) – 34 г/моль

3.     Составляем пропорцию

8*27 г алюминия при взаимодействии дают 3*34 г сероводорода

108 г алюминия при взаимодействии дают Х г сероводорода

4.     51 г сероводорода составляет 100%

35 г сероводорода составляет Х%

Х = 35*100/51 =68,63%

Answer 2

Calculation of Hydrogen Sulfide Mass

To calculate the mass of hydrogen sulfide (H2S) produced when 108 g of aluminum reacts with concentrated sulfuric acid (H2SO4) upon heating, we need to consider the balanced chemical equation for the reaction. Unfortunately, the search results provided do not directly give the balanced equation for this reaction. However, we can still proceed with the calculation using the given information.

Let's assume that the reaction between aluminum and sulfuric acid produces hydrogen gas (H2) and aluminum sulfate (Al2(SO4)3). The balanced equation for this reaction can be written as:

2 Al + 3 H2SO4 -> 3 H2 + Al2(SO4)3

According to the given information, the yield or the percentage of the reaction is 75%. This means that only 75% of the maximum possible amount of hydrogen sulfide is produced.

To calculate the mass of hydrogen sulfide, we need to determine the molar mass of H2S. Hydrogen (H) has a molar mass of approximately 1 g/mol, and sulfur (S) has a molar mass of approximately 32 g/mol. Therefore, the molar mass of H2S is approximately 34 g/mol.

Now, let's calculate the theoretical yield of hydrogen sulfide using the molar ratio between H2S and Al:

1 mol Al produces 1 mol H2S

Since the molar mass of Al is approximately 27 g/mol, we can calculate the number of moles of Al:

108 g Al * (1 mol Al / 27 g Al) = 4 mol Al

Since the molar ratio between Al and H2S is 1:1, the number of moles of H2S produced is also 4 mol.

Next, we need to calculate the mass of H2S using the molar mass:

4 mol H2S * (34 g H2S / 1 mol H2S) = 136 g H2S

However, we need to consider the yield of the reaction, which is 75%. Therefore, the actual mass of H2S produced is:

136 g H2S * 0.75 = 102 g H2S

Therefore, the mass of hydrogen sulfide produced when 108 g of aluminum reacts with concentrated sulfuric acid with a 75% yield is approximately 102 grams.

Please note that the balanced chemical equation assumption made in this calculation may not be accurate without the actual balanced equation. It is always recommended to refer to reliable sources or consult a chemistry expert for precise calculations.