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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) H2NCONH2(s) + H2O(g) Ammonia gas at 223°C and 90. atm flows into a reactor at a rate of 670. L/min. Carbon dioxide at 223°C and 47 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?

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1. Convert NH3 and CO2 to STP using the Combined Gas Law. 1. NH3: P1V1T2 = P2V2T1 90atm x 670L x 273K = 1atm x V2 x 496K V2 = (90 x 670 x 273) ÷ 496 NH3 vol. at STP = 16,461,900 ÷ 496 = 33,189L 1 mole at STP = 22.4L 33,189 ÷ 22.4 = 1,482 moles = 1,482g/min 2. CO2: 47atm x 600L x 273K = 1atm x V2 x 496K V2 = (47 x 600 x 273) ÷ 496 CO2 vol. at STP = 7,698,600 ÷ 496 = 15,521L 15,521 ÷ 22.4 = 693 moles = 693g/min Total mass of Urea produced: = 1,482g + 693g = 2.175kg/min