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Serhud [2]
3 years ago
14

The production of ethylbenzene, a very popular industrial chemical, is carried out reacting benzene with ethylene in liquid phas

e. This reaction takes place in a series of reactors that involve multiple side reactions and intermediates. Ethylene, being the limiting reactant, is used up first and hence a considerable amount of benzene remains unreacted. From one of the reactors in the series, the exit stream is a mixture of this unreacted benzene (1), an intermediate – toluene (2), and the product ethyl benzene (3).
It is desirable to separate this liquid mixture before sending the components to the next series of reactors/process steps. So 100 mol/min of this mixture is flashed from 200 mm Hg and 50 °C to 100 mm Hg. If the mole fraction of benzene and toluene are 40% each when the mixture enters the flash distillation unit, determine if the mixture will flash completely, partially, or not at all. Assume ideal gas and ideal solution behavior for the vapor phase and liquid phase, respectively. If the mixture does flash partially, determine the composition and molar flow rates of the equilibrium streams exiting the reactor. Show all calculations by hand using your preferred method for solving simultaneous equations. Alternatively, you may use Solver (Excel) but this must be accompanied by a printout of a neatly formatted Excel sheet showing your equations and constraints.

Chemistry
1 answer:
gogolik [260]3 years ago
3 0

Answer:

Explanation:

CHECK BELOW ATTACHMENT FOR THE SOLUTION

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What is the difference between a mixture and a compound? (need an easy two sentence answer (able to explain it to a 8 your old).
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2 years ago
Given the balanced equation representing a reaction occurring in an electrolytic cell:
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4 0
3 years ago
Read 2 more answers
I need help with this, please :00000
mojhsa [17]

theoretical yield of the reaction is 121.38 g of NH₃ (ammonia)

limiting reactant is N₂ (nitrogen)

excess reactant is H₂ (hydrogen)

Explanation:

We have the following chemical reaction:

N₂ + 3 H₂ → 2 NH₃

Now we calculate the number of moles of each reactant:

number of moles = mass / molar weight

number of moles of N₂ = 100 / 28 = 3.57 moles

number of moles of H₂ = 100 / 2 = 50 moles

From the chemical reaction we see that 3 moles of H₂ are reacting with 1 moles of N₂, so 50 moles of H₂ are reacting with 16.66 moles of N₂ but we only have 3.57 moles of  N₂ available, so the limiting reactant will be N₂ and the excess reactant will be H₂.

Knowing the chemical reaction and the limiting reactant we devise the following reasoning:

if          1 mole of N₂ produce 2 moles of NH₃

then    3.57 moles of N₂ produce X moles of NH₃

X = (3.57 × 2) / 1 = 7.14 moles of NH₃

mass = number of moles × molar weight

mass of NH₃ = 7.14 × 17 = 121.38 g

theoretical yield of the reaction is 121.38 g of NH₃

Learn more about:

limiting reactant

brainly.com/question/13979150

#learnwithBrainly

4 0
3 years ago
what is the maximum number of covalent bonds that an oxygen atom with atomic number 8 can make with hydrogen? question 4 options
Oliga [24]

Maximum number of covalent bonds that an oxygen atom can make with hydrogen is 2.

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  • There are no longer any empty orbitals in the octet of oxygen after it is complete. As a result, it is unable to accept more electrons or create more bonds.

Therefore, Oxygen can only generate two bonds because it needs two additional electrons to complete its octet, after which it will run out of empty orbitals in which to receive additional electrons and create additional bonds.

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3 0
1 year ago
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