16. A. A B. C. D. E. 17. A. B. C. D. E. 18. A. B. C. D. E. For the reaction 2NO2(g) + Cl2(g) = 2NO₂Cl(g), the following

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16 A A B C D E 17 A B C D E 18 A B C D E For The Reaction 2no2 G Cl2 G 2no Cl G The Following 1 (83.89 KiB) Viewed 23 times

16. A. A B. C. D. E. 17. A. B. C. D. E. 18. A. B. C. D. E. For the reaction 2NO2(g) + Cl2(g) = 2NO₂Cl(g), the following mechanism has been proposed: NO₂(g) + Cl₂(g) NO₂Cl(g) + CI(g)...(1) (SLOW) NO₂(g) + Cl(g) = NO₂Cl(g). (2) Based upon this mechanism and the information supplied it can be inferred that: the intermediate in this mechanism is NO₂Cl(g) the rates of consumption of NO₂(g) and Cl₂(g) in (1) are greater than those of NO₂(g) and Cl(g) in (2) the consumption and production of NO₂(g) in (1) are the rate determining steps the rate of formation of Cl(g) in (1) is greater than the rate of consumption of NO₂(g) in (2) the overall reaction order is three. Which one of the following statements is correct? The value of the equilibrium constant is affected by the presence of a catalyst. Increasing the volume of a gaseous equilbrium mixture causes the system to shift in the direction that decreases the number of moles of gas. A large value of Kc indicates that the equilibrium mixture contains more reactants than products. When the reaction quotient (Q) is greater than the equilibrium constant (Kc), the reaction will form more products. Equilibrium for which all substances are in the same phase is called homogeneous equilibrium. Carbon dioxide (CO₂) is formed according to the following equation: 2CO(g) + O2(g) = 2CO₂(g) 0.690 mol of CO₂ were placed into a 600 cm³ flask with 0.330 mol of O₂ and the reaction was allowed to equilibrate. At equilibrium it was found that 0.360 mol of CO₂ were present. How many moles of CO and O₂ were in the flask at equilibrium? 0.550 moles CO and 0.825 moles O2 0.550 moles CO and 1.10 moles O₂ 0.330 moles CO and 0.495 moles O₂ 0.330 moles CO and 0.600 moles O2 0.550 moles CO and 0.330 moles O₂