Problem Set #7 – Chapter 16 – Chemical Equilibrium1. The equilibrium constant for the reaction,H2(g) + I2(g) == 2 HI(g) is 54.9 at 699.0 K (Kelvin).4 HI(g) == 2 H2(g) + 2 I2(g) under the same...

Problem Set #7 – Chapter 16 – Chemical Equilibrium1. The equilibrium constant for the reaction,H2(g) + I2(g) == 2 HI(g) is 54.9 at 699.0 K (Kelvin).4 HI(g) == 2 H2(g) + 2 I2(g) under the same conditions?A. -109.8B. 0.00911C. 109.8D. 0.0182E. 0.000332Note: the == indicates the equilibrium double arrow2. Using this data,2 NO(g) + Cl2(g) == 2 NOCl(g)NO2(g)== NO(g) + ½ O2(g)Kc = 3.20 X 10-3Kc = 3.93calculate a value for Kc for the reaction,NOCl (g) + ½ O2 (g) == NO2 (g) + ½ Cl2 (g)A. 20.2B. 2.06 X 10-4C. 4.49D. 4.84 X 10-3E. 0.2233. The equilibrium constant, Kc for the system,CaO(s) + CO2(g) == CaCO3(s), isA. Kc =C. Kc =D. Kc =E. Kc =[CaO] [CO2] / [CaCO3][CaCO3]/[CaO](CaCO3] / [CaO] [CO2]1 / [CO2]B. Kc = ICO2]4. For the reaction, 2 SO2(g) + O2(g) == 2 SO3(g), at 450.0 K (Kelvin) the equilibriumconstant, Kc, has a value of 4.62. A system was charged to give these initialconcentrations, [SO3] = 0.254 M and [O2] = 0.00855 M, and [SO2] = 0.500 M. Inwhich direction will it go?A. to the rightB. to the leftC. it will remain at the same concentrationsD. not enough data to tell5. For the reaction system, 2 H2O(g) + O2(g) == 2 H2O2 (g), the equilibriumconcentrations are[H2O2] = 0.120 M; [H2O] = 0.860 M; [O2] = 0.330 M.Calculate the value of Kc for this reaction.A. 0.423B. 0.872C. 0.0590D. 1.31E. 2.516. For the reaction system, 2 SO2(g) + O2(g) = 2 SO3(g), Kc hasa value of 4.62 at 450.0 K (Kelvin). A system, at equilibrium has the followingconcentrations:[SO3] = 0.254 M; [O2] = 0.00855 M. What is the equilibrium concentration ofSO2?A. 2.75 MB. 1.63 MC. 2.66 MD. 0.612 ME. 1.28 M7. A study of the system, H2(g) + I2(g) == 2 HI(g), was carriedout. Kc = 54.9 at 699.0 K (Kelvin) for this reaction. A system was charged with2.50 moles of HI in a 5.00 liter vessel as the only component initially. The systemwas brought up to 699.0 K and allowed to reach equilibrium. How many moles ofH2 should there be in the container at that time?A. 1.97 molesB. 0.337 molesC. 0.394 molesD. 0.266 molesE. 0.0531 moles8. The reaction, 2 SO3(g) == 2 SO2(g) + O2(g) is endothermic.Predict what will happen if the temperature is increased.A. the pressure decreasesB. more SO3(g) is producedC. Kc increasesD. Kc decreasesE. none of the above9. For the system CaO(s) + CO2(g) = CaCO3(s), I added 1.00 mol of CaO(s) to 1.00L of0.500M CO2(g) at 200 oC. At equilibrium the [CO2] = 0.150M. What is the value of Kpfor this reaction?A. 0.172B. 0.150C. 5.82D. 6.67E. 2.5910. Look at problem 26 on page 754 of the text. Which of the four choices wouldproduce more products in the reaction? The choices are:A.B.C.D.E.only one of thesechoices (a) and (b)choices (c) and (d)choices (a), (b), and (c)all four choices