Question

На 30.0 30.0 г яичной скорлупы подействовали 100 100 мл столового уксуса. Какой максимальный объем газа (при н.у. в литрах с точностью до десятых) мог при этом выделиться? Испарением уксуса и воды пренебречь. Столовый уксус — — 9% 9 % ‑ный водный раствор одноосновной уксусной кислоты, имеющей формулу CH3COOH CH 3 COOH , плотность столового уксуса составляет 1.01 1.01 г/мл. Выделившийся газ перекачали в предварительно вакуумированный сосуд объемом 5 5 л. Какую долю (в процентах) от объема сосуда займет газ?

Answer 1

Ответ:

2CH3COOH+CaCO3=Ca(CH3COO)2+CO2+H2O

m(CH3COOH)=100*0.09*1.01=9,09 грамм

n(CH3COOH)=9.09/60,05=0,1513 моль

n(CaCO3)=30/100=0,3 моль

Ведем расчет выхода по карбонату

m(CO2)=0,3*44,01=13,203 грамм

V(CO2)=0.3*22.4=6,72 литра

Answer 2

Ответ:

В первом 6.72 а второй вопрос в процентах 93

Объяснение:

Answer 3

Calculation of Maximum Gas Volume

To calculate the maximum volume of gas that can be released when 100 ml of vinegar (9% acetic acid solution) reacts with 30.0 g of eggshell, we need to consider the reaction between acetic acid and calcium carbonate in the eggshell.

The balanced chemical equation for this reaction is:

2 CH3COOH + CaCO3 → Ca(CH3COO)2 + H2O + CO2

From the equation, we can see that 2 moles of acetic acid react with 1 mole of calcium carbonate to produce 1 mole of carbon dioxide gas.

To determine the number of moles of acetic acid, we can use the formula:

moles = mass / molar mass

The molar mass of acetic acid (CH3COOH) is approximately 60.05 g/mol.

Using the given mass of vinegar (100 ml) and its density (1.01 g/ml), we can calculate the mass of acetic acid:

mass of acetic acid = volume of vinegar x density of vinegar = 100 ml x 1.01 g/ml = 101 g

Now, we can calculate the number of moles of acetic acid:

moles of acetic acid = mass of acetic acid / molar mass of acetic acid = 101 g / 60.05 g/mol ≈ 1.68 mol

Since the reaction ratio between acetic acid and calcium carbonate is 2:1, we can conclude that 1.68 moles of acetic acid will react with 0.84 moles of calcium carbonate.

To calculate the volume of carbon dioxide gas produced, we can use the ideal gas law:

PV = nRT

Where: - P is the pressure (at standard conditions, it is 1 atm) - V is the volume of the gas - n is the number of moles of the gas - R is the ideal gas constant (0.0821 L·atm/(mol·K)) - T is the temperature (at standard conditions, it is 273.15 K)

Since we are interested in the volume of gas at standard conditions (n. u.), we can rearrange the equation as:

V = nRT / P

Substituting the values:

V = 0.84 mol x 0.0821 L·atm/(mol·K) x 273.15 K / 1 atm ≈ 18.3 L

Therefore, the maximum volume of gas that can be released is approximately 18.3 liters.

Calculation of Gas Fraction in the Vessel

To calculate the fraction of gas in the vessel, we need to compare the volume of the gas to the total volume of the vessel.

Given that the vessel has a volume of 5 liters and the gas volume is 18.3 liters, we can calculate the gas fraction as follows:

Gas fraction = (gas volume / total volume) x 100%

Gas fraction = (18.3 L / 5 L) x 100% ≈ 366%

Therefore, the gas will occupy approximately 366% of the total volume of the vessel.

Please note that the calculated gas fraction exceeds 100% because the gas volume is larger than the vessel's volume.