please answer these questions Given the following complex reaction mechanism for the reaction H2(g) + Br2(g)...
5. For the overall exothermic reaction: H2(g) + Br2(g) → 2HBr(g) the following mechanism was determined: fast Equilibrium Step 1: Brz(8) 2Br(g) Step 2: H2(g) + Br(g)_52HBr(g) + H(g) Step 3: H(g) + Br(g) k3 HBr(g) slow fast Use a plot of AH versus Reaction Pathway to illustrate the three step reaction profile.
Provide a mechanism for the following reaction. Br2, hv H2 H2 CH - HBr H2 H2 H3C Br
At 700 K, Kc = 1.56×10–2 for the reaction 2 HBr(g) ⇌ H2(g) + Br2(g). In a given experiment, 0.050 mol of H2, and 0.050 mol Br2 are introduced into a 5.0-L flask. What is the equilibrium concentration of HBr?
1) Consider the following reaction at equilibrium: H2(g) + Br2(g) = 2 HBr(g) Kc = 3.8 x 104 a) Is this reaction reactant-favored or product-favored? (1 point) Answer: b) Based on the given equilibrium reaction, determine the value of the equilibrium constant for the following reaction: Show your work for full credit! (4 points) 2 HBr(g) = H2(g) + Br2(g) Kc = c) Use both the equation and your answer from Part b to answer the problem. In a 1.00...
In Section 29-7, McQuarrie details the chain reaction between H2(g) and Br2(g). Consider the realted chain reaction H2(g) + Cl2(g) → 2HCl(g). The mechanism for this reaction is: Cl2(g) + Mg) = 2 Cl(g) +Mg) ki CI(g) + H2(g) → HCI(g) + H() k2 H(g) + Cl2(8) = HCI(g) + CI(8) k3 2Cl(g) + Mg) = Cl2(g) + Mg) ks (a) Use bond dissociation energies to explain why it is reasonable to exclude the analogous inhibition steps in this mechanism...
Consider the following reaction mechanism: 1) Initiation Br2 → 2 Br• 2) Propagation (here a cycle of two steps) Br• + H2 → HBr + H• H• + Br2 → HBr + Br• 3) Termination 2 Br• → Br2 This reaction is catalyzed by platinum. My question is what does the platinum do? I know that platinum is able to split the H2 bond but is that the only function of the platinum in this reaction?
33. Consider the reaction: H2(g) + Br2(g) → 2 HBr (9) The graph shows the concentration of Br, as a function of time. 0.85 M Concentration (M) 068 ML 15s... Br To 0 50 100 150 a. Use the graph to calculate each quantity: i. the average rate of the reaction between 0 and 25 s ii. the instantaneous rate of the reaction at 25 s iii. the instantaneous rate of formation of HBr at 25
35) Given the equilibrium reaction at constant pressure: 2HBr(g) + 72.7 kJ = H2(g) + Br2(g) When the temperature is increased, the equilibrium will shift to the A) left, and the concentration of HBr(g) will decrease B) right, and the concentration of HBr(g) will decrease C) right, and the concentration of HBr(g) will increase D) left, and the concentration of HBr(g) will increase
At 700 K, Kc = 1.56-10-2 for the reaction 2 HBr(g) + H2(g) + Br2(c). In a given experiment, 0.050 mol of H2 and 0.050 mol Br2 are introduced into a 5.0-L fiask. What is the equilibrium concentration of HBr? Multiple Choice О оо16 м o O o.250 м o O o125 м o О 31-10-3 м o О 7,8*10-3 м
Enter your answer in the provided box. You are given the following data: H2(g) → 2H(g) Br2(g) → 2Br(g) AH = 436.4 kJ/mol AH = 192.5 kJ/mol H2(g) + Br2(g) → 2HBr(g) AH = -72.4 kJ/mol Calculate Ahº for the reaction H(g) + Br(g) — HBr(g) kJ/mol