Question

Этилен объёмом 100л (н.у.) нагрели в присутствии металлического катализатора. Образовавшуюся смесь газов пропустили через бромную воду. Масса непоглотившегося газа составила 6,4г. Рассчитайте массу ацетилена, который образовался из этилена, и выход продукта реакции дегидрирования.

Answer 1

Этилен представляет собой бесцветный газ, обладающий слабым, едва ощутимым запахом. Уже при температурах выше 350 градусов С этилен частично разлагается на метан и ацетилен:

3С2Н4 = 2СН4 + 2С2Н2

CH=CH +2Br2 = CHBr2-CHBr2

m(СH4)=6,4г

n(ch4)=6,4/16=0,4

n(ch4)=n(c2h2)=0,4

m(c2h2)=M*n=0,4*26=10,4

M(c2h2)=2Ar(c)+2Ar(h)=26

Answer 2

Calculation of the Mass of Acetylene and Yield of the Reaction

To calculate the mass of acetylene formed from ethylene and the yield of the dehydrogenation reaction, we need to use the information provided.

Given: - Volume of ethylene: 100 L (at standard temperature and pressure, n.у.) - Mass of unreacted gas: 6.4 g

To find the mass of acetylene formed, we can use the stoichiometry of the reaction. The balanced equation for the dehydrogenation of ethylene to acetylene is:

C2H4(g) -> C2H2(g)

From the equation, we can see that one mole of ethylene (C2H4) reacts to form one mole of acetylene (C2H2).

To calculate the number of moles of ethylene, we can use the ideal gas law:

PV = nRT

Where: - P is the pressure (at standard temperature and pressure, n.у., it is 1 atm) - V is the volume of the gas (100 L) - n is the number of moles of the gas (to be determined) - R is the ideal gas constant (0.0821 L·atm/(mol·K)) - T is the temperature in Kelvin (n.у. is 273 K)

Solving for n, we have:

n = PV / RT

Substituting the values, we get:

n = (1 atm) * (100 L) / (0.0821 L·atm/(mol·K) * 273 K)

Calculating this, we find that the number of moles of ethylene is approximately 4.03 moles.

Since the reaction is stoichiometric, the number of moles of acetylene formed will be the same as the number of moles of ethylene reacted. Therefore, the mass of acetylene formed can be calculated using the molar mass of acetylene (C2H2), which is approximately 26 g/mol:

Mass of acetylene = Number of moles of acetylene * Molar mass of acetylene = 4.03 moles * 26 g/mol ≈ 104.78 g

Therefore, the mass of acetylene formed from ethylene is approximately 104.78 grams.

To calculate the yield of the reaction, we can use the following formula:

Yield = (Mass of acetylene formed / Mass of ethylene used) * 100

Substituting the values, we have:

Yield = (104.78 g / 6.4 g) * 100 ≈ 1637.81%

Therefore, the yield of the dehydrogenation reaction is approximately 1637.81%.

Please note that the values provided in the search snippet are not sufficient to calculate the mass of acetylene or the yield of the reaction. The given information does not include the mass of ethylene used or the conditions of the reaction.