At 500°C, hydrogen iodide decomposes according to 2HI(g) => H2(g) +12(g) For HI(g) heated to 500°C in a 1.00 L reaction vessel, chemical analysis determined these concentrations at equilibrium: [H2] = 0.407M, [I2] = 0.407M, and [HI] = 3.44M. If an additional 1.00 mol of HI(g) is introduced into the reaction vessel, what are the equilibrium concentrations after the new equilibrium has been reached? [HI] = [H₂] = 2 [12] =

At 37.0 °C, the reaction CO2(g) + H2O(l) ⇔ H+(aq) + HCO3-(aq) has K = 2.94x10-8. If PCO2 = 5.25 mbar, [H2O] = 55.5 mol L-1, and [H+] = 47.1 µmol L-1 at equilibrium, determine the concentration of [HCO3-] in µmol L-1.

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7. An initial mixture of 5.00 M N2 and 5.00 M H2 is placed in a reaction vessel and allowed to come to equilibrium. The equi- librium concentration of the NH3 is determined to be 2.00M. Determine K for the reaction below. N2(g) + 3H2(8) = 2NH3(g) (A) 0.125 (B) 0.250 (C) 0.500 (D) 1.00

A mixture of 2.75e-02 mol of O, 4.32e-02 mol of NOCI, 7.25e-02 mol of NO, and 7.59e-03 mol of Cly is placed in a 1.0-L steel pressure vessel at 1654 K. The following equilibrium is established: Ox(9) + 2 NOCI(9) =2 NO;(0) + Ch(9) At equilibrium 6.01e-03 mol of Clz is found in the reaction mixture. Calculate the equilibrium pressures of all gases in the reaction vessel and the value of Kp for the reaction. Pick the correct statement from the multiple choices, Use the value R= 0.0821 L-atm/mal-K for the gas constant. Oa) The equilibrium pressure of NOCI is PNoc 6.29 atm. O b) The equilbrium pressure of O2 is Po, 3.52 atm. O9 The equilbrium constant is Kp 9.2e-02. O4) The equibrum constant is Kp 2.2e+00. Oe) The equilibrium pressure of NO is PNo, 10.3 atm.

The equilibrium constant for the synthesis of ammonia N2(g) + 3 H2(g) --> 2 NH3(g) has the value K = 3.19 × 10^-4 at  400°C. Calculate the equilibrium partial pressures of N2(g), H2(g), and NH3(g) if the total pressure is 1.00 atm and the H:N atomratio in the system is 3;1. (Hint: Try the approximationthat PN2  and PH2  > PNH3  and see if the resulting equationsare simpliied.)

Al(OH),(s) = Al³*(aq) +30H¯(aq) X x.- +. log, Cos, K = [AF][OH]; ОН

The equilibrium constant K. for the equation CS2 (9) + 4H, (9) # CH4 (9) + 2H, S(g9) at 900°C is 27.8. What is the value of K. for the following equation? | CH, (9)+1H2 S(9) = Cs, (9)+2Hz (9) Ke

Bromine monochloride is synthesized using the reaction Br, (g) + Cl, (g) = 2 BrC(g) K, = 1.1 x 104 at 150 K A 201.0 L flask initially contains 0.951 kg of Br, and 1.116 kg of Cl,. Calculate the mass of BrCI, in grams, that is present in the reaction mixture at equilibrium. Assume ideal gas behavior. mass of BrCl: What is the percent yield of BrCl? percent yield:

At 1200 K in the presence of solid carbon, an equilibrium mixture of CO and CO2 (called “producer gas") contains 98.3 mol percent CO and 1.69 mol percent of CO2 when the total pressure is 1 atm. The reaction is CO2(g) + C(graphite) 2 2 CO(g) (a) Calculate Pco and Pco;. (b) Calculate the equilibrium constant. (c) Calculate AG° for this reaction.