Question

Из ацетилена объемом 61,6 л (н.у.) по реакции Кучерова было получено 72,6 г уксусного альдегида. Определите выход продукта реакции в % от теоретически возможного. Помогите , пожалуйста с задачкой)))) буду очень рада и благодарна!) сижу час и не получается решить ..

Answer 1

61,6л              m(теор)-?
C2H2+H2O=CH3CHO
22,4л            44г
m( теор.CH3CHO)=61,6*144/22,4=396(г)
η=m(прак)*100%/m(теор)
η(CH3CHO)=72,6*100/396=18,33%
Ответ:18,33%

Answer 2

Calculation of the Reaction Yield

To determine the yield of the reaction, we need to compare the amount of acetic aldehyde obtained to the theoretical amount that could be produced from the given volume of acetylene.

The balanced equation for the reaction of acetylene to acetic aldehyde is:

2 C2H2 + H2O → CH3CHO

According to the equation, 2 moles of acetylene (C2H2) react with 1 mole of water (H2O) to produce 1 mole of acetic aldehyde (CH3CHO).

To calculate the theoretical yield of acetic aldehyde, we need to convert the given volume of acetylene to moles using the ideal gas law. The ideal gas law equation is:

PV = nRT

Where: - P is the pressure of the gas (in atm) - V is the volume of the gas (in liters) - 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 of the gas (in Kelvin)

Given: - Volume of acetylene = 61.6 L (at standard temperature and pressure, n.у.)

Since the temperature is not provided, we will assume it to be 273 K (standard temperature).

Using the ideal gas law, we can calculate the number of moles of acetylene:

n = PV / RT

Substituting the values: - P = 1 atm (standard pressure) - V = 61.6 L - R = 0.0821 L·atm/mol·K - T = 273 K

n = (1 atm * 61.6 L) / (0.0821 L·atm/mol·K * 273 K)

Calculating n: - n ≈ 2.38 moles

According to the balanced equation, 2 moles of acetylene react to produce 1 mole of acetic aldehyde. Therefore, the theoretical yield of acetic aldehyde can be calculated as:

Theoretical yield = (2.38 moles acetylene) / 2 * (molar mass of acetic aldehyde)

The molar mass of acetic aldehyde (CH3CHO) is approximately 44.05 g/mol.

Calculating the theoretical yield: - Theoretical yield ≈ (2.38 moles / 2) * 44.05 g/mol - Theoretical yield ≈ 52.29 g

Now, we can calculate the percentage yield of the reaction by comparing the actual yield (72.6 g) to the theoretical yield (52.29 g):

Percentage yield = (actual yield / theoretical yield) * 100

Calculating the percentage yield: - Percentage yield ≈ (72.6 g / 52.29 g) * 100 - Percentage yield ≈ 138.9%

Therefore, the yield of the reaction is approximately 138.9% of the theoretical yield.

Please note that a yield above 100% is not physically possible. There might be errors in the experimental procedure or measurements that led to a higher than expected yield.