QUESTION 2 Consider the following reaction and its equilibrium constant: 12(g) + Br2(g) = 2 IBr(g) Kc=1.1 x 102 A reaction mixture contains 0.51 M 12, 0.27 M Br2 and 3.5 M IBr. Which of the following statements is TRUE concerning this system? OA. The reaction quotient will decrease. OB. The reaction will shift in the direction of reactants. OC. The system is at equilibrium. OD. The reaction will shift in the direction of products. O E. The equilibrium constant will decrease.

:Br: slow Br fast a) Write the rate law for the reaction above. b) Draw curved arrows showing electron movement in each step, and label the step as nucleophilic attack, proton transfer, leaving group, or rearrangement. c) How would the reaction rate be affected if the iodide concentration were doubled? d) How would the reaction rate be affected if the 2-bromo-2-methylpentane concentration were doubled?

At a certain temperature, Keq for the following reaction between sulfur dioxide and nitrogen dioxide is 4.8.   SO2(g)   +   NO2(g)   ↔   NO(g)   +   SO3(g)   SO2(g) and NO2(g) have the same initial concentration:   0.36 mol/L.  What amount of SO3(g) is present in a 5.0 L container at equilibrium?

Consider the following reaction at equilibrium:2SO2(g) + O2 (g) <==> 2SO3(g)Determine if the following changes will increase, decrease or not affect the partial pressure of SO2.a. Decreasing the amount of oxygen in the systemb. Decreasing the volume of the systemc. Decreasing the temperature of the systemd. Decreasing the pressure of the systeme. Adding a catalyst to the reaction system

Consider the reaction 2NO (g) + Cl2 (g) → 2NOCI (g), for which Kc = 6.50 × 104 at 35° C. If the starting concentrations of NO, Cl2 and NOCI are 3.60x103 M, 1.25 M and 5.87 M respectively, in which direction will the reaction proceed to reach equilibrium? a. Depends on the pressure Ob. To the right C. To the left d. The reaction is already at equilibrium

3. Determine the reaction quotient and predict the direction that each of the following reactions will proceed to reach equilibrium: Keq = 4.6 × 10¹ a. A 1.00 L flask containing 0.0500 mol NO (g), 0.0155 mol Cl₂ (g), and 0.500 mol NOCI(g): 2NO(g) + Cl₂(g) = 2NOCI(g) A: shift right b. A 5.00 L flask containing 14 g N₂ (g), 12 g H₂ (g), and 17 g NH3(g): N₂(g) + 3H₂(g) = 2NH3(g) Keq = 0.060 (at 526 °C) c. A 2.00 L flask containing 230 g SO3 (8) 2SO3(g) = 2SO₂(g) + O₂(8) Keq = 0.230 A: shift left A: shift right

Write the equilibrium expressions for the following reactions a. 3 Fe (s) + 4 H20 (g) Fe304 (s) + 4 H2 (g) b. 2 SO2 (g) + 02 (g)= 2 SO3 (g)

Consider the following reaction: 2HI(g) → H₂(g) + 1₂ (9) If 2.74 moles of HI(g), 0.333 moles of H₂, and 0.588 moles of I2 are at equilibrium in a 10.3 L container at 878 K, the value of the equilibrium constant, Кси is

For the following chemical reaction,      CO (g)   +   H2O (g)      CO2 (g)   +   H2 (g)     Kc = 0.0257 If a 2.00L vessel is charged with 0.200 moles of CO, 1.13 moles of H2O, 0.199 moles of CO2, and 0.175 moles of H2, what is the equilibrium concentration of CO?     a. 0.610M   b. 0.054M   c. 0.264M   d. 0.0451M   e. 0.145M