Question

Вычислить массу соли, полученную растворением 1.3г цинка в соляной кислоте.

Answer 1

Дано:
m(Zn)=1.3г
Найти:
m(ZnCl₂)-?
Решение:
Zn+2HCl=ZnCl₂+H₂
M(Zn)=65г/моль
n(Zn)=m/M=1.3/65=0.02моль
По реакции:
n(Zn)=n(ZnCl₂)=0.02моль
M(ZnCl₂)=136г/моль
m(ZnCl₂)=n*M=0.02*136=2.72г
Ответ:2,72г

Answer 2

Calculation of the Mass of Salt Obtained by Dissolving 1.3g of Zinc in Hydrochloric Acid

To calculate the mass of salt obtained by dissolving 1.3g of zinc in hydrochloric acid, we need to consider the chemical reaction that occurs between zinc and hydrochloric acid. The balanced chemical equation for this reaction is as follows:

Zn + 2HCl → ZnCl2 + H2

From the balanced equation, we can see that 1 mole of zinc reacts with 2 moles of hydrochloric acid to produce 1 mole of zinc chloride and 1 mole of hydrogen gas.

To calculate the mass of zinc chloride produced, we need to determine the molar mass of zinc chloride (ZnCl2). The molar mass of zinc (Zn) is approximately 65.38 g/mol, and the molar mass of chlorine (Cl) is approximately 35.45 g/mol. Since there are two chlorine atoms in zinc chloride, the molar mass of zinc chloride is:

Molar mass of ZnCl2 = (65.38 g/mol) + 2*(35.45 g/mol) = 136.28 g/mol

Now, we can calculate the number of moles of zinc used in the reaction:

Number of moles of zinc = mass of zinc / molar mass of zinc Number of moles of zinc = 1.3 g / 65.38 g/mol ≈ 0.0199 mol

According to the balanced equation, the molar ratio between zinc and zinc chloride is 1:1. Therefore, the number of moles of zinc chloride produced is also approximately 0.0199 mol.

Finally, we can calculate the mass of zinc chloride produced:

Mass of zinc chloride = number of moles of zinc chloride * molar mass of zinc chloride Mass of zinc chloride = 0.0199 mol * 136.28 g/mol ≈ 2.71 g

Therefore, the mass of salt obtained by dissolving 1.3g of zinc in hydrochloric acid is approximately 2.71 grams.

Please note that the values provided in this response are approximate and may vary slightly depending on the actual molar masses used.