1. An industrial chemist is studying the rate of the Haber synthesis: N2 + 3H2 →...
1. An industrial chemist is studying the rate of the Haber synthesis: N2 + 3H2 → 2NH3. Starting with a closed reactor containing 1.15 mol/L of N2 and 0.20 mol/L of H2, she finds that the H2 concentration has fallen to 0.10 mol/L after 20. seconds. What is the average rate of reaction of H2 over this time? (Enter in mol/liter/sec).
2. What is the average rate of NH3 production for this example? (Enter in mol/liter/sec).
3. Estimate the N2 concentration after 30 seconds? (Enter in mol/liter).
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1. An industrial chemist is studying the rate of the Haber
synthesis: N2 + 3H2 →...
An industrial chemist is studying the rate of the Haber synthesis: N2 + 3H2 ? 2NH3....
An industrial chemist is studying the rate of the Haber synthesis: N2 + 3H2 ? 2NH3. Starting with a closed reactor containing 1.00 mol/L of N2 and 0.30 mol/L of H2, she finds that the H2 concentration has fallen to 0.16 mol/L after 30. seconds. What is the average rate of reaction of H2 over this time? (Enter in mol/liter/sec). What is the average rate of NH3 production for this example? (Enter in mol/liter/sec). Estimate the N2 concentration after 25...
An industrial chemist is studying the rate of the Haber synthesis: N2 + 3H2 → 2NH3....
An industrial chemist is studying the rate of the Haber synthesis: N2 + 3H2 → 2NH3. Starting with a closed reactor containing 1.25 mol/L of N2 and 0.35 mol/L of H2, she finds that the H2 concentration has fallen to 0.14 mol/L after 20. seconds. What is the average rate of reaction of H2 over this time? (Enter in mol/liter/sec). What is the average rate of NH3 production for this example? (Enter in mol/liter/sec). Estimate the N2 concentration after 20...
Chapter 13, Question 14 Parameterization A chemist is studying the rate of the Haber synthesis: N2...
Chapter 13, Question 14 Parameterization A chemist is studying the rate of the Haber synthesis: N2 + 3H2 2 NH3 Starting with a closed reactor containing 1.25 mol/L of N2 and 0.50 mol/L of Hz, the chemist finds that the H2 concentration has fallen to 0.25 mol/L in 27 seconds. What is the relative rate of reaction over this time? the tolerance is +/-29 LINK TO TEXT What is the average rate of NH3 production? the tolerance is +/-2% What...
Chapter 13, Question 14 Parameterization A chemist is studying the rate of the Haber synthesis: N2...
Chapter 13, Question 14 Parameterization A chemist is studying the rate of the Haber synthesis: N2 + 3H2 2 NH3 Starting with a closed reactor containing 1.25 mol/L of N, and 0.50 mol/L of H7, the chemist finds that the Hy concentration has fallen to 0.25 mol/L in 46 seconds. What is the relative rate of reaction over this time? M/S the tolerance is +/-2% What is the average rate of NH3 production? M/S the tolerance is +/-2% LINK TO...
Consider the Haber synthesis of gaseous NH3 (ΔH∘f = -46.1 kJ/mol; ΔG∘f = -16.5 kJ/mol): N2(g)+3H2(g)→2NH3(g)...
Consider the Haber synthesis of gaseous NH3 (ΔH∘f = -46.1 kJ/mol; ΔG∘f = -16.5 kJ/mol): N2(g)+3H2(g)→2NH3(g) What are the equilibrium constants Kp and Kc for the reaction at 350 K ? You may assume that ΔH∘ and ΔS∘ are independent of temperature.
4) Synthesis of ammonia by the Haber process occurs by the reaction N2(g) + 3H2(8) 52NH3(8)...
4) Synthesis of ammonia by the Haber process occurs by the reaction N2(g) + 3H2(8) 52NH3(8) Species ah(kJ mol-1) 4S(J mol-1 K-1) H2(g) 0 130.7 N2(g) 0 191.6 NH3(g) -46.1 192.5 Assuming that AH and 45 are essentially unchanged in the temperature ranging from 25 °C to 400 °C: a. Calculate K at 25°C. b. Calculate K at 400C. (R = 8.314 J mol-1 K-1)
The reaction for the Haber process, the industrial production of ammonia, is N2(g) + 3 H2(g)...
The reaction for the Haber process, the industrial production of ammonia, is N2(g) + 3 H2(g) + 2 NH3(g) Assume that under certain laboratory conditions ammonia is produced at the rate of 2.98 x 10-5 mol L-15-1. At what rate is nitrogen consumed? At what rate is hydrogen consumed? N2 is consumed at the rate of mol L-15-1 H2 is consumed at the rate of mol L-15-1
Question 8 1 pts The Haber process for the production of ammonia is the main industrial...
Question 8 1 pts The Haber process for the production of ammonia is the main industrial process of producing ammonia today. Prior to developing this process, ammonia was difficult to produce on an industrial scale. The reaction for the Haber process is: N2(g) + 3H2(g) = 2 NH3(g). Using the following values, determine the equilibrium constant for this reaction at 25°C. Substance AGR°(kJ/mol) N H2 NH3 - 16.4 Enter your answer to three significant figures.
In the Haber process, ammonia is synthesized from nitrogen and hydrogen: N2(g) + 3H2(g) → 2NH3(g) ΔG° at 298 K for thi...
In the Haber process, ammonia is synthesized from nitrogen and hydrogen: N2(g) + 3H2(g) → 2NH3(g) ΔG° at 298 K for this reaction is -33.3 kJ/mol. The value of ΔG at 298 K for a reaction mixture that consists of 1.9 atm N2, 1.6 atm H2, and 0.65 atm NH3 is ________. -3.86 × 103 -1.8 -7.25 × 103 -104.5 -40.5
Reaction: 3H2(g)+N2(g) ---> 2NH3(g) If the reaction above is first order with respect to N2 and...
Reaction: 3H2(g)+N2(g) ---> 2NH3(g) If the reaction above is first order with respect to N2 and the reaction rate is 0.040 mol/L*s when the concentration of N2 is 0.10 mol/L what is the reaction rate if the concentration is increased to .20 mols/L? Assume [H2] remains constant.
Chapter 13, Question 14 Parameterization A chemist is studying the rate of the Haber synthesis: N2 + 3H2 2 NH3 Starting with a closed reactor containing 1.25 mol/L of N2 and 0.50 mol/L of Hz, the chemist finds that the H2 concentration has fallen to 0.25 mol/L in 27 seconds. What is the relative rate of reaction over this time? the tolerance is +/-29 LINK TO TEXT What is the average rate of NH3 production? the tolerance is +/-2% What...
Chapter 13, Question 14 Parameterization A chemist is studying the rate of the Haber synthesis: N2 + 3H2 2 NH3 Starting with a closed reactor containing 1.25 mol/L of N, and 0.50 mol/L of H7, the chemist finds that the Hy concentration has fallen to 0.25 mol/L in 46 seconds. What is the relative rate of reaction over this time? M/S the tolerance is +/-2% What is the average rate of NH3 production? M/S the tolerance is +/-2% LINK TO...
4) Synthesis of ammonia by the Haber process occurs by the reaction N2(g) + 3H2(8) 52NH3(8) Species ah(kJ mol-1) 4S(J mol-1 K-1) H2(g) 0 130.7 N2(g) 0 191.6 NH3(g) -46.1 192.5 Assuming that AH and 45 are essentially unchanged in the temperature ranging from 25 °C to 400 °C: a. Calculate K at 25°C. b. Calculate K at 400C. (R = 8.314 J mol-1 K-1)
The reaction for the Haber process, the industrial production of ammonia, is N2(g) + 3 H2(g) + 2 NH3(g) Assume that under certain laboratory conditions ammonia is produced at the rate of 2.98 x 10-5 mol L-15-1. At what rate is nitrogen consumed? At what rate is hydrogen consumed? N2 is consumed at the rate of mol L-15-1 H2 is consumed at the rate of mol L-15-1
Question 8 1 pts The Haber process for the production of ammonia is the main industrial process of producing ammonia today. Prior to developing this process, ammonia was difficult to produce on an industrial scale. The reaction for the Haber process is: N2(g) + 3H2(g) = 2 NH3(g). Using the following values, determine the equilibrium constant for this reaction at 25°C. Substance AGR°(kJ/mol) N H2 NH3 - 16.4 Enter your answer to three significant figures.
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