Question

Через 80 г 20% -го раствора гидроксида натрия пропустили углекислый газ до образования карбоната натрия. Вычислите объём (н. у.) затраченного на реакцию газа.

Answer 1

Ответ:

получится 100% объёма углекислого газа

Объяснение:

....

Answer 2

Calculation of Gas Volume Used in the Reaction

To calculate the volume of gas used in the reaction, we need to consider the given information:

- 80 g of a 20% solution of sodium hydroxide (NaOH) was used. - Carbon dioxide gas (CO2) was passed through the solution until sodium carbonate (Na2CO3) was formed.

To calculate the volume of gas used, we need to convert the mass of sodium hydroxide to moles and then use the stoichiometry of the reaction to determine the moles of carbon dioxide produced.

1. Convert the mass of sodium hydroxide to moles: - The molar mass of sodium hydroxide (NaOH) is 40 g/mol (22.99 g/mol for Na + 16.00 g/mol for O + 1.01 g/mol for H). - The given mass of sodium hydroxide is 80 g. - Therefore, the number of moles of sodium hydroxide is calculated as follows:

moles of NaOH = mass of NaOH / molar mass of NaOH moles of NaOH = 80 g / 40 g/mol moles of NaOH = 2 mol

2. Use the stoichiometry of the reaction to determine the moles of carbon dioxide produced: - The balanced chemical equation for the reaction is: 2 NaOH + CO2 → Na2CO3 + H2O - From the balanced equation, we can see that 1 mole of carbon dioxide reacts with 2 moles of sodium hydroxide. - Therefore, the number of moles of carbon dioxide produced is half the number of moles of sodium hydroxide:

moles of CO2 = 1/2 * moles of NaOH moles of CO2 = 1/2 * 2 mol moles of CO2 = 1 mol

3. Convert the moles of carbon dioxide to volume using the ideal gas law: - The ideal gas law equation is: PV = nRT where P is the pressure, V is the volume, n is the number of moles, R is the ideal gas constant, and T is the temperature. - Since the pressure, temperature, and gas constant are not given, we cannot calculate the exact volume of the gas. However, we can assume standard temperature and pressure (STP) conditions, which are 0°C (273.15 K) and 1 atm (101.3 kPa) respectively. - At STP, 1 mole of any ideal gas occupies 22.4 liters