Initial concentration of H2 and Br2 are 2.0M each. After 15 seconds the concentration of Br2 is 1.72M, find the rate of reaction.
H2(aq) + Br2(aq) --> 2HBr
Initial concentration of H2 and Br2 are 2.0M each. After 15 seconds the concentration of Br2...
The Kc of the reaction H2 (g)+Br2 (g)=2HBr (g) is 2.18×10+6. If the initial concentration of HBr in 12.0L vessel is 3.20 moles, calculate the concentration of H2, Br2 and HBr at equilibrium. Use ICE table. Show calculations and all work & may have to use quadratic equation.
Consider the following reaction: H2(g)+Br2(g)→2HBr(g) The graph below shows the concentration of Br2 as a function of time.(Figure 1) Make a rough sketch of a curve representing the concentration of HBr as a function of time. Assume that the initial concentration of HBr is zero.
consider the reaction; 2HBr yeilds H2 + Br2, if the volume of the reactionwith the average rate of the reaction being .0017, what amount of Br2 moles was formed during the first 18 sec of the reaction
please answer these questions Given the following complex reaction mechanism for the reaction H2(g) + Br2(g) → 2 HBr (g): Br2 → 2 Brº (rate constant ka) Br + H2 → HBr +H* (rate constant kb) Hø + Br2 → HBr + Br" (rate constant ke) H + HBr → H2 + Brº (rate constant kd) Br + Brº Br2 (rate constant ke) Which of the following is true? The rate constant for the termination step is ka. The steady-state...
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
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
The equilibrium constant for the following reaction: H2(g) + Br2(g) ↔ 2HBr (g) is 1.20 x 103 at a certain temperature. Find the equilibrium pressure of HBr if 9.20 atm of HBr is introduced into a sealed container at this temperature.
The equilibrium constant for the following reaction: H2(g) + Br2(g) ↔ 2HBr (g) is 1.35 x 103 at a certain temperature. Find the equilibrium pressure of HBr if 5.70 atm of HBr is introduced into a sealed container at this temperature.
The equilibrium constant for the following reaction: H2(g) + Br2(g) ↔ 2HBr (g) is 1.90 x 103 at a certain temperature. Find the equilibrium pressure of HBr if 14.50 atm of HBr is introduced into a sealed container at this temperature.
Consider the reaction A2 + B2 ⇌ 2AB. If the initial concentration of both A2 and B2 is 4.0 M, and after 10 minutes the reaction appears to stop. The concentration of [A2] is now 2.0M. d. We can discuss the rate in terms of [A2], [B2], or [AB]. How are they related to each other? - Δ[A2]/Δt = e. What is the difference between Δ[A2]/Δt and d[A2]/dt ? f. At t = 15 minutes has the reaction actually...