Question

Сколько литров углекислого газа выделится при взаимодействии соляной кислоты с 4г карбоната кальция, если выход составит 90% от теоретически возможного?

Answer 1

Ответ на фотографии

Answer 2

Calculation of the Amount of Carbon Dioxide Produced

To calculate the amount of carbon dioxide (CO2) produced when hydrochloric acid (HCl) reacts with calcium carbonate (CaCO3), we need to consider the balanced chemical equation for the reaction:

2HCl + CaCO3 -> CaCl2 + CO2 + H2O

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

To find the number of moles of calcium carbonate, we can use the given mass of 4 grams and the molar mass of calcium carbonate, which is approximately 100.09 g/mol.

Number of moles of CaCO3 = mass of CaCO3 / molar mass of CaCO3 Number of moles of CaCO3 = 4 g / 100.09 g/mol Number of moles of CaCO3 = 0.03996 mol (approximately)

Since the reaction has a 90% yield, we need to calculate 90% of the theoretical moles of carbon dioxide produced.

Number of moles of CO2 = 90% of (2 * number of moles of CaCO3) Number of moles of CO2 = 0.9 * (2 * 0.03996 mol) Number of moles of CO2 = 0.07192 mol (approximately)

To convert the number of moles of carbon dioxide to liters, we can use the ideal gas law, assuming standard temperature and pressure (STP). At STP, 1 mole of any ideal gas occupies 22.4 liters.

Volume of CO2 = number of moles of CO2 * 22.4 L/mol Volume of CO2 = 0.07192 mol * 22.4 L/mol Volume of CO2 = 1.609088 L (approximately)

Therefore, approximately 1.61 liters of carbon dioxide will be produced when 4 grams of calcium carbonate reacts with hydrochloric acid, with a yield of 90% of the theoretical amount.

Please note that the above calculation assumes ideal conditions and may not account for other factors that could affect the reaction.