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.
Assuming same volume, 2 moles will be produced per mole of reactant, giving the following behavior.
Consider the following reaction: H2(g)+Br2(g)→2HBr(g) The graph below shows the concentration of Br2 as a function...
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 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 reaction 2HBr(g) H2(g) Br2(1) The standard free energy change for this reaction is 107.0 kJ. The free energy change when 2.50 moles of HBr(g) react at standard condition is kJ. What is the maximum amount of useful work that the reaction of 2.50 moles of HBr(g) is capable of producing in the surroundings under standard conditions? If no work can be done, enter none. kJ Consider the reaction 2HBr(g) H2(g) Br2(1) The standard free energy change for this...
10. The equilibrium constant Kc for the reaction H2(g) + Br2(g) ⇆ 2HBr(g) is 2.180 × 106 at 730°C. Starting with 2.20 moles of HBr in a 13.7−L reaction vessel, calculate the concentrations of H2, Br2, and HBr at equilibrium. [H2] = [Br2] = [HBr] =
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
The equilibrium constant Kc for the reaction H2(g) + Br2(g) ⇆ 2HBr(g) is 2.180 × 106 at 730°C. Starting with 1.20 moles of HBr in a 21.3−L reaction vessel, calculate the concentrations of H2, Br2, and HBr at equilibrium.
For the reaction H2(g) + Br2(g) → 2HBr(g) Kp = 3.6 x 104 at 1494 K. What is the value of Kp for the following reaction at 1494 K? 42 H2(g) + / Br2(g) HBr(g) K". p Submit
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.