Consider the reaction 2 D(g) + 3 E(g) + F(g) 2 G(g) + H(g). When [E] is decreasing at 0.10 mol/ L-s, how fast is [D] decreasing? (Disregard the use of any negative sign.) 0.30 mol/ L-s 0.15 mol/ L-s None of these 0.10 mol/ L-s 0.067 mol/ L:s

The elementary reactionearnin2H, 0(g ) = 2H2(g) + 02(8)millanproceeds at a certain temperature until the partial pressures of H, O, H2, and O, reach 0.0350 atm, 0.00600 atm, and = 0.00500 atm, respectively. What is the value of the equilibrium constant at this temperature?

4. Sketch a graphical representation of the following events for the equilibrium below. PCIse 5 PCe + Cl ΔΗ = + 88 kJ/mol 15(g) 3(g) 2(g) a) PCI, is introduced into a flask at t=0 to a concentration of 2 mol/L. b) The flask is heated gently until no further changes in concentration of PCl, occur (5 minutes). At this time, the concentration of PCl(g) is 1.25 mol/L. c) At t=10 min an additional 0.25 mol/L of chlorine gas is injected into the flask. d) At t=15 min, no further changes in concentration were observed. Indicate the places on the graph where the system is at equilibrium. f) Use the information provided to calculate K, the equilibrium constant of this reactions. Conc'n (mol/L) Time (min)

the phosgene dissociation reaction follows the reaction equation: COCl2 (g) -> CO(g) + Cl2(g). delta H = + 420 kj/mol   In the above reaction the following actions are given: 1. pressure lowered 2. the temperature is raised 3. Volume down things that can increase the concentration of phosgene in equilibrium?

The following reaction has been allowed to come to equilibrium in a 2.0L container: 1. 2 Cl2 (g) + O2 (g) + energy 2 Cl20 (g) 11 State the direction in which the equilibrium would be shifted (Right, Left or Unchanged) upon application of each of the following "stresses": Shift (R. L, or U "Stress" Increase the concentration of Cl20 a) b) Increase the concentration of 02 c) Decrease the concentration of Cl2 d) Increase the pressure by decreasing the volume to 1.0 L e) Increase the temperature f) Add a catalyst g) Add He (g) to the 1.0 L container

ONLY LOOKING FOR THE ANSWER TO PART B. I already got part one!

+ Imagine 212. mmol of HCH,CO, are removed from a flask containing a mixture of HCH,CO,, H,O, H,O' and CH,CO, at equilibrium, and then answer the following questions. Zero. What is the rate of the forward Greater than zero, but less than the rate of the reverse reaction. reaction before any HCH3CO2 has been removed from the flask? Greater than zero, and equal to the rate of the reverse reaction. Greater than zero, and greater than the rate of the reverse reaction. Zero. What is the rate of the forward Greater than zero, but less than the rate of the reverse reaction. reaction just after the HCH3CO2 has been removed from the flask? Greater than zero, and equal to the rate of the reverse reaction. Greater than zero, and greater than the rate of the reverse reaction. Zero. What is the rate of the forward Greater than zero, but less than the rate of the reverse reaction. reaction when the system has again reached equilibrium? Greater than zero, and equal to the rate of the reverse…

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Chapter 16 (Due 06/10, 23:00) O Saved 3 attempts left Check my work Be sure to answer all parts. Consider the following equilibrium process at 686°C: So CO;(g) + H2(g) = CO(g)+ H2O(g) Guidec The equilibrium concentrations of the reacting species are [CO] = 0.0500 M, [H2] = 0.0420 M, [CO2] = 0.0900 M, and [H,O] = 0.0350 M. ok (a) Calculate K, for the reaction at 686°C. int (b) If we add CO, to increase its concentration to 0.480 mol / L, what will the concentrations of all the gases be when equilibrium is reestablished? ences CO2: M H,: M CO: M H,O: M МaсВook Pro Thank We @ #3 $ 4. 5. 8. CO 3. 2.

Determine how the following changes affect the given equilblirium reaction that is held in a closed container.       A(g) + 2 B(s) ⇌ 3 C(g) + 3 D(s)      ΔH°rxn = −0.25 kJ/mol Adding some A(g)    Adding some D(s)    Removing some C(g)    Increasing the temperature    Halving the volume of the container        The following mechanism is proposed for the reaction  2 A2 + B2  →  2 C  A2 + B2  →  R + C  slow  A2 + R  →  C   fast  What is the rate law for the overall reaction?            A. rate = k[A2]   B. rate = k[A2]2 [B2]   C. rate = k[A2]2   D. rate = k[R]2    E. rate = k[A2][B2]