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 seconds? (Enter in mol/liter).
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...
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...
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...
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.
The Haber reaction for the manufacture of ammonia is: N2 + 3H2 → 2NH3 Without doing any experiments, which of the following can you say MUST be true? The reaction is not an elementary reaction. The activation energy is positive. Disappearance rate of N2 = 3 (Disappearance rate of H2). Δ[H2]/Δt will have a positive value. Disappearance rate of H2 = 3 (Disappearance rate of N2). Reaction rate = -Δ[N2]/Δt. The reaction is first order in N2.
The Haber reaction for the manufacture of ammonia is: N2 + 3H2 → 2NH3 Without doing any experiments, which of the following can you say MUST be true? True False The reaction is not an elementary reaction. True False The reaction is first order in N2. True False Δ[H2]/Δt will have a positive value. True False Reaction rate = -Δ[N2]/Δt. True False Disappearance rate of N2 = 3 (Disappearance rate of H2). True False Disappearance rate of H2 = 3 (Disappearance rate of N2). True False The...
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
Calculate KC in terms of molar concentration for the reaction N2(g) + 3H2(g) 2NH3(g) when the equilibrium concentration moles per liter are: N2 = 0.02, H2 = 0.01, NH3 = 0.10.
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.