Question

При взаимодействии известняка массой 30 г с массовой долей примесей в нем 5% с соляной кислотой выделился газ. Определите объём выделившегося газа

Answer 1

Дано:
m(CaCO3)=30 г(5% примесей)
Найти:
V(газа)=?

Решение:
CaCO3+2HCl=CaCl2+CO2+H2O
в известняке 5%, тогда:
m(CaCO3)=30x0.95=28.5(г)
M(CaCO3)=100 г/моль, Vm=22.4 л/моль
V(CO2)=x л
28.5/100=x/22.4
x=6.384
Ответ: V(CO2)=6.384(л).

Answer 2

Task:

Calculate the volume of gas released when 30g of limestone with 5% impurities reacts with hydrochloric acid.

Solution:

To calculate the volume of gas released when 30g of limestone with 5% impurities reacts with hydrochloric acid, we can use the chemical reaction equation for the reaction between limestone and hydrochloric acid. The reaction can be represented as:

CaCO3(s) + 2HCl(aq) → CaCl2(aq) + H2O(l) + CO2(g)

From the reaction equation, we can see that 1 mole of calcium carbonate (CaCO3) reacts with 2 moles of hydrochloric acid (HCl) to produce 1 mole of carbon dioxide (CO2) gas.

First, we need to calculate the moles of calcium carbonate in 30g of limestone, taking into account the 5% impurities.

The molar mass of CaCO3 is 100.09 g/mol.

The moles of CaCO3 can be calculated using the formula: moles = mass / molar mass

The moles of CaCO3 in 30g of limestone can be calculated as: moles = 30g / 100.09 g/mol

Let's calculate the moles of CaCO3 first.

Calculation:

The moles of CaCO3 in 30g of limestone: moles = 30g / 100.09 g/mol moles ≈ 0.2997 moles

Now, since 1 mole of CaCO3 produces 1 mole of CO2, the moles of CO2 produced will also be approximately 0.2997 moles.

The volume of gas can be calculated using the ideal gas law equation: PV = nRT

Where: P = pressure V = volume n = number of moles R = ideal gas constant T = temperature

Assuming standard temperature and pressure (STP), the volume of gas can be calculated using the molar volume of a gas at STP, which is approximately 22.4 L/mol.

Result:

The volume of gas released when 30g of limestone with 5% impurities reacts with hydrochloric acid is approximately 6.72 L at STP.

Note:

The actual volume of gas released may vary depending on the specific conditions of the reaction.