Homework Answers
N2(g) + 3H2(g) -----> 2NH3(g)
From above equation,
1 mol N2 = 2 mol NH3
Number of moles of NH3 generated from 50 moles of N2 gas is,
50 mol N2 × ( 2 mol NH3 / 1 mol N2)
= 100 mol NH3
Hence the correct option is (A) 100 mol
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The Haber-Bosch process is a very important industrial process. In the Haber-Bosch process, hydrogen gas reacts...
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The Haber process for production of ammonia is as follows: N2 (g) + 3H2(g) → 2NH3 (g) An experiment ran this process using 5.75 moles of N2 and excess hydrogen gas. The reaction produced 7.50 moles of NH3. Calculate the percent yield for this experiment. Round your answer to the nearest whole number. Do not use scientific notation. Do not include the percent sign!
7. Most of the industrial ammonia today is produced via the Haber Process. The Chemical reaction is one we've seen many times now: N20g) +3H2(g)-2NH3(g) If 20 moles of ammonia (NH3) are needed for a particular process, how many moles of diatomic Nitrogen (N2) are needed?
Figure 1 represents the flow diagram of the production of ammonia from hydrogen and nitrogen (Haber process), according to the following reaction at 400°C and atmospheric pressure: N2(g) + 3H2(g) + 2NH3(9) TN).6 TH).6 7 Yis 1,6 = 9.7 6 5TH = 0 kmol h-1 3 TH(a). T.1 ANN (9) TIN2(g) 4 = 1,623.4 = 0 kmol h-1 Figure 1. Flow diagram for question 1. The process is designed for a target production of 200 kmol h of pure ammonia....
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