Urea (h2nconh2) is used extensively as a nitrogen source in fertilizers. it is produced commercially from the reaction of ammonia and carbon dioxide.

2 nh3(g) + co2(g) reaction arrow identifying the need for heat and pressure to be applied h2nconh2(s) + h2o(g)

ammonia gas at 223°c and 90. atm flows into a reactor at a rate of 580. l/min. carbon dioxide at 223°c and 48 atm flows into the reactor at a rate of 600. l/min. what mass of urea is produced per minute by this reaction assuming 100% yield?

The mass of urea produced is 2.175kg/min

Explanation:

Step 1: The balanced equation

2 NH3(g) + CO2(g) → H2NCONH2(s) + H2O(g)

Step 2: Given data

Ammonia gas (NH3) at 223°C (= and 90 atm flows into a reactor at a rate of 580 L/min

Carbon dioxide( CO2) at 223°C and 48 atm flows into the reactor at a rate of 600. L/min.

Step 3: Calculate

⇒NH3:

(P1*V1)/ T1 = (P2*V2)/T2

P1 = 90 atm

V1 = 670L

T1 = 496 K

P2 = 1 atm

V2 = TO BE DETERMINED

T2= 273K

P1V1T2 = P2V2T1

90atm*670L*273K = 1atm*V2*496K

V2 = (90 x 670 x 273)/496

V2 = 33189 L ( Volume at STP)

At STP 1 mole = 22.4 L

This means 33,189/22.4 = 1,482 moles

This gives us a rate of 1482g /min NH3

CO2:

P1 = 47 atm

V1 = 600L

T1 = 496 K

P2 = 1 atm

V2 = TO BE DETERMINED

T2= 273K

47atm*600L*273K = 1atm*V2*496K

V2 = (47*600*273) /496

V2 = 15,521L

15,521 ÷ 22.4 = 692.92 moles = 692.92g/min

1482g /min NH3 + 692.92g/min = 2.175kg/min

sorry idk the answer well to you i have a explaination

explanation: a formula which shows the arrangement of atoms in the molecule of a compound