Question

Вариант 141 Распределите вещества по классам, назовите вещества:CaO, ZnCL2, HNO2, Br2O7, Ba(OH)2, H3PO4, FeI2, NaNO2, Al2(CO3)3, PbO2 Даны вещества: оксид меди, нитрат меди, барий, вода, гидроксид цинка. Какие из этих веществ будут взаимодействовать с азотной кислотой? 3 Напишите уравнения соответствующих реакций 3 Осуществите цепочку превращений:O2 H2O  H2 HCl4 Рассчитайте массу осадка, образовавшегося при взаимодействии 9.8 г серной кислоты с раствором хлорида бария

Answer 1

1.CaO-оксид кальция.(Класс-оксиды)

ZnCl2-хлорид цинка(Класс-соли)

HNO2-азотная кислота(Класс-кислоты)

Br2O7-окид брома(кислотный оксид) Класс-Оксиды

Ba(OH)2-гидроксид бария (Класс-Соли)

H3PO4-Фосфорная кислота(Класс-Кислоты)

FeI-Иодит железа (Класс-Соли)

NaNO2-Нитрат натрия(Класс-Соли)

Al2(CO3)3-Карбонат алюминия(Класс-Соли)

PbO-Оксид свинца(Основной оксид) Класс-Оксиды.

2.CuO+2HNO3=Cu(NO3)2+H2O(об.)

CuNO3+HNO3= Не взаимодействует.

Ba+2HNO3=Ba(NO3)2+H2(з.)

H20+HNO3= Не взаимодействует.

Zn(OH)2+2HNO3=Zn(NO3)2+2H2O(об.н)

3.O2-H2O-H2-HCl

1)O2+2H2=2H2O(c.)

2)H2O=2H2+O2(p.)

3)H2+2Cl=2HCl(c.)

4.Расчёт по химическим уравнениям.

H2SO4+BaCl2=BaSO4+2HCl

n=m/M; M=Mr;

Mr(H2SO4)= Ar(H)*2+Ar(S)+Ar(O)*4= 2*1+32+16*4=98.

M(H2SO4)=98г/моль.

n(BaSO4)=x.

x=0,1*1/1=0,1.

n(BaSO4)=0,1 моль.

m=M*n.

Mr(BaSO4)=Ar(Ba)+Ar(S)+Ar(O)*4=138+32+64=234.

M(BaSO4)=234г/моль.

m(BaSO4)=0,1 моль*234г/моль=23,4г.

Ответ:23,4г.

Answer 2

Classification of Substances:

To classify the given substances, let's identify their chemical formulas and determine their classes.

1. CaO: Calcium oxide is an ionic compound, also known as a metal oxide. 2. ZnCl2: Zinc chloride is an ionic compound, also known as a metal halide. 3. HNO2: Nitrous acid is a weak acid. 4. Br2O7: Bromine heptoxide is a covalent compound, also known as a nonmetal oxide. 5. Ba(OH)2: Barium hydroxide is an ionic compound, also known as a metal hydroxide. 6. H3PO4: Phosphoric acid is a strong acid. 7. FeI2: Iron(II) iodide is an ionic compound, also known as a metal halide. 8. NaNO2: Sodium nitrite is an ionic compound, also known as a metal nitrite. 9. Al2(CO3)3: Aluminum carbonate is an ionic compound, also known as a metal carbonate. 10. PbO2: Lead(IV) oxide is an ionic compound, also known as a metal oxide.

Interaction of Substances with Nitric Acid:

To determine which of the given substances will react with nitric acid (HNO3), we need to consider their chemical properties. Nitric acid is a strong acid and can react with certain substances.

The substances that will react with nitric acid are: - ZnCl2: Zinc chloride will react with nitric acid to form zinc nitrate and hydrochloric acid. The balanced equation for this reaction is: ``` ZnCl2 + 2HNO3 -> Zn(NO3)2 + 2HCl ```

- Al2(CO3)3: Aluminum carbonate will react with nitric acid to form aluminum nitrate, carbon dioxide, and water. The balanced equation for this reaction is: ``` Al2(CO3)3 + 6HNO3 -> 2Al(NO3)3 + 3CO2 + 3H2O ```

Transformation Chain: O2 -> H2O -> H2 -> HCl4

The given transformation chain involves the conversion of oxygen (O2) to water (H2O), then to hydrogen gas (H2), and finally to tetrachloromethane (HCl4).

1. O2 to H2O: Oxygen gas reacts with hydrogen gas in the presence of a catalyst to form water. The balanced equation for this reaction is: ``` 2H2 + O2 -> 2H2O ```

2. H2O to H2: Water can be decomposed into hydrogen gas and oxygen gas through a process called electrolysis. The balanced equation for this reaction is: ``` 2H2O -> 2H2 + O2 ```

3. H2 to HCl4: Hydrogen gas can react with chlorine gas to form tetrachloromethane (HCl4). The balanced equation for this reaction is: ``` CH4 + 4Cl2 -> CCl4 + 4HCl ```

Calculation of Precipitate Mass:

To calculate the mass of the precipitate formed when 9.8 g of sulfuric acid (H2SO4) reacts with a solution of barium chloride (BaCl2), we need to determine the limiting reactant and use stoichiometry.

The balanced equation for the reaction between sulfuric acid and barium chloride is: ``` H2SO4 + BaCl2 -> BaSO4 + 2HCl ```

From the balanced equation, we can see that the mole ratio between sulfuric acid and barium sulfate is 1:1. This means that 1 mole of sulfuric acid reacts with 1 mole of barium sulfate.

To find the limiting reactant, we need to compare the number of moles of sulfuric acid and barium chloride. The molar mass of sulfuric acid (H2SO4) is 98.09 g/mol, and the molar mass of barium chloride (BaCl2) is 208.23 g/mol.

The number of moles of sulfuric acid can be calculated using its molar mass: ``` moles of H2SO4 = mass of H2SO4 / molar mass of H2SO4 = 9.8 g / 98.09 g/mol = 0.1 mol ```

The number of moles of barium chloride can be calculated using its molar mass: ``` moles of BaCl2 = mass of BaCl2 / molar mass of BaCl2 = unknown (not provided) ```

Since the mass of barium chloride is not provided, we cannot determine the number of moles of barium chloride and, therefore, cannot determine the limiting reactant or calculate the mass of the precipitate.

Please provide the mass of barium chloride to proceed with the calculation.