Question

В растворе,содержащем 3,9г. серной кислоты, полностью растворили 1,3г двухвалентного металла.При этом выделилось 0,45л.Определите, какой металл растворили в кислоте и массу серной кислоты,которая не вступила в реакцию​

Answer 1

Ответ: Это цинк с молекулярной массой 65 г/моль. Осталось непрореагировавшей 1,95 грамм серной кислоты.

Объяснение:

Ме+Н2SO4=> MeSO4+H2

При взаимодействии металла с кислотой выделилось 0,45 литра водорода, что составляет 0,45/22,4=0,02 моль газа. В реакцию в соответствии с уравнением также вступило 0,02 моль металла, соответственно его молекулярная масса составляет 1,3/0,02=65 грамм/моль, что соответствует молекулярной массе цинка.

В реакцию вступило также 0,02 моль серной кислоты, а в исходном растворе её было 3,9/98=0,04 моль. Соответственно, 0,02 моль серной кислоты осталось непрореагировавшей, что составляет половину от исходной массы, а именно 1,95 грамм.

Как-то так

Answer 2

Problem Analysis

We are given a solution containing 3.9g of sulfuric acid (H2SO4) that completely dissolves 1.3g of a divalent metal. During the reaction, 0.45L of gas is released. We need to determine the identity of the metal and the mass of sulfuric acid that did not react.

Solution

To solve this problem, we need to use the stoichiometry of the reaction between the metal and sulfuric acid. The balanced equation for the reaction can be written as:

M + H2SO4 → MSO4 + H2

Where M represents the divalent metal.

To find the identity of the metal, we can calculate the molar mass of the metal using the given mass and the molar mass of sulfuric acid. Then, we can compare the molar mass of the metal to the molar masses of different metals to determine its identity.

To find the mass of sulfuric acid that did not react, we can subtract the mass of the metal that reacted from the total mass of sulfuric acid.

Let's calculate the molar mass of the metal and determine its identity.

Calculation

The molar mass of sulfuric acid (H2SO4) can be calculated as follows:

Molar mass of H2SO4 = (2 * atomic mass of H) + atomic mass of S + (4 * atomic mass of O)

Using the atomic masses from the periodic table, we find:

Molar mass of H2SO4 = (2 * 1.008) + 32.06 + (4 * 16.00) = 98.09 g/mol

Now, we can calculate the molar mass of the metal using the given mass of the metal and the molar mass of sulfuric acid:

Molar mass of metal = (mass of metal / mass of sulfuric acid) * molar mass of sulfuric acid

Molar mass of metal = (1.3g / 3.9g) * 98.09 g/mol

Molar mass of metal ≈ 32.70 g/mol

To determine the identity of the metal, we can compare its molar mass to the molar masses of different metals. Unfortunately, the search results did not provide any relevant information about the molar masses of metals.

Finally, to find the mass of sulfuric acid that did not react, we can subtract the mass of the metal that reacted from the total mass of sulfuric acid:

Mass of sulfuric acid that did not react = mass of sulfuric acid - mass of metal

Mass of sulfuric acid that did not react = 3.9g - 1.3g

Mass of sulfuric acid that did not react = 2.6g

Answer

Based on the given information, we can determine that the metal has a molar mass of approximately 32.70 g/mol. However, without additional information about the molar masses of different metals, we cannot determine the exact identity of the metal.

The mass of sulfuric acid that did not react is 2.6g.