The fresh feed to an ammonia production process contains N2 and H2 in stoichiometric proportion, along...

The fresh feed to an ammonia production process contains N2 and H2 in stoichiometric proportion, along with an inert gas (I). The feed is combined with a recycle stream containing the same three species, and the combined stream is fed to a reactor in which a low single-pass conversion of N2 is achieved. The reactor effluent flows to a condenser. A liquid stream containing essentially all of the NH3 formed in the reactor and a gas stream containing all the inerts and the unreacted N2 and H2 leave the condenser. The gas stream is split into two fractions with the same composition: one is removed from the process as a purge stream, and the other is the recycle stream combined with the fresh feed. In every stream containing N2 and H2, the two species are in stoichiometric proportion. The mole fraction of inerts in the fresh feed is 0.01, the single-pass conversion of N2 (and H2) in the reactor is 0.2, and the fraction of gas leaving the condenser that is purged (mol purged/mol total) is 0.1. Taking a 1 mole fresh feed basis, find the composition of each stream in the process and the overall conversion of N2.

Solutions

Expert Solution

Amanda K answered 1 year ago

Next > < Previous

Related Solutions

Chemical Engineering problem. The fresh feed to an ammonia synthesis plant contains 24.30% N 2 ,...

Chemical Engineering problem. The fresh feed to an ammonia synthesis plant contains 24.30% N 2 , 75.20% H 2 and 0.50% Ar. The reaction in the reactor is not complete so that recycle is necessary. In a specific operation, the fresh feed is mixed with recycled gases and the mixture is sent to the reactor. The gases leaving the reactor are sent to a cooler-condenser from which pure liquid ammonia is obtained. The gas stream from the cooler-condenser also includes...

(a) Write a stoichiometric table for the reaction N2 + 3 H2  2 NH3 for...

(a) Write a stoichiometric table for the reaction N2 + 3 H2  2 NH3 for an isothermal, isobaric flow system with equimolar (or equal molar) feeds of N2 & H2. (b) If the entering total pressure is 16.4 atm and the entering temperature is 1727 oC, calculate the concentration of hydrogen and nitrogen entering the reactor. (c) Plot the gas composition (molar fractions) as a function of the conversion. Is there anything worth noticing? Can you explain it? What...

An equilibrium mixture of N2, H2 and NH3 at 700K contains 0.036M H2 and 0.015M H2....

An equilibrium mixture of N2, H2 and NH3 at 700K contains 0.036M H2 and 0.015M H2. At this temperature, Kc for the reation N2(g)+3H2(g) <> 2NH3(g) is 0.29. What is the concentration of NH3?

Methanol (CH3OH) is produced by reacting carbon monoxide (CO) and hydrogen (H2). A fresh feed stream...

Methanol (CH3OH) is produced by reacting carbon monoxide (CO) and hydrogen (H2). A fresh feed stream containing CO and H2 joins a recycle stream and the combined stream is fed into a reactor. The reactor outlet stream flows at a rate of 350 mol/min and contains 10.6 wt% H2, 64.0 wt% CO, and 25.4 wt% CH3OH. The stream enters a cooler in which most of the methanol is condense. The liquid methanol is withdrawn as a product, and the gas...

Hydrogen gas, H2, reacts with nitrogen gas, N2, to form ammonia gas, NH3, according to the...

Hydrogen gas, H2, reacts with nitrogen gas, N2, to form ammonia gas, NH3, according to the equation 3H2(g)+N2(g)→2NH3(g) Part B How many grams of NH3 can be produced from 2.15 mol of N2 and excess H2. Part C How many grams of H2 are needed to produce 13.02 g of NH3? Part D How many molecules (not moles) of NH3 are produced from 4.83×10−4 g of H2? Express your answer numerically as the number of molecules.

Hydrogen gas, H2, reacts with nitrogen gas, N2, to form ammonia gas, NH3, according to the...

Hydrogen gas, H2, reacts with nitrogen gas, N2, to form ammonia gas, NH3, according to the equation 3H2(g)+N2(g)→2NH3 How many grams of H2 are needed to produce 10.70 g of NH3? How many molecules (not moles) of NH3 are produced from 3.21×10−4 g of H2?

Hydrogen gas, H2, reacts with nitrogen gas, N2, to form ammonia gas, NH3, according to the...

Hydrogen gas, H2, reacts with nitrogen gas, N2, to form ammonia gas, NH3, according to the equation 3H2(g)+N2(g)→2NH3(g) 1a. How many grams of NH3 can be produced from 2.60 mol of N2 and excess H2 1b. How many grams of H2 are needed to produce 11.32 g of NH3? 1c. How many molecules (not moles) of NH3 are produced from 4.06×10−4 g of H2?

Hydrogen gas, H2, reacts with nitrogen gas, N2, to form ammonia gas, NH3, according to the...

Hydrogen gas, H2, reacts with nitrogen gas, N2, to form ammonia gas, NH3, according to the equation 3H2(g)+N2(g)→2NH3(g) a. How many grams of H2 are needed to produce 11.70 g of NH3? b. How many molecules (not moles) of NH3 are produced from 4.42×10−4 g of H2?

Acetylene is hydrogenated to form ethane. The feed to the reactor contains 1.50 mol H2 /mol...

Acetylene is hydrogenated to form ethane. The feed to the reactor contains 1.50 mol H2 /mol C2H2. Write the stoichiometric equation for this reaction, and then answer the following questions: 1) Calculate the stoichiometric reactant ratio of hydrogen to acetylene (mol H2 / mol C2H2). 2)Identify the limiting reactant, and then calculate the percentage by which the other reactant is in excess. 3) Calculate the extent of reaction, assuming all of the limiting reactant is consumed. Use a basis of...

Subjects