An empty 5.00-L flask is charged with 0.300 g of pure H,S(9), at 25 °C. Ammonium bisulfide, NH,HS, forms ammonia, NH3, and hydrogen sulfide, H2S, through the reaction NH, HS(s) = NH3(9) + H2S(9) Part A This reaction has a K value of 0.120 at 25 °C. Evaluate the validity of the following statements. Drag each item to the appropriate bin. • View Available Hint(s) Reset Help The reaction proceeds to the left. Qis greater than K. No reaction occurs. Qis equal to 0. The pressure of ammonia is zero. The reaction proceeds to the right. True False Submit Part B What is the initial pressure of H2S(g) in the flask? Express your answer numerically in bars. • View Available Hint(s) P = bar Submit

The equilibrium constant, Kc, for the following reaction is 1.29x10-2 at 600 K. coCI,(g) ? CO(g) + Cl2(g) Calculate the equilibrium concentrations of reactant and products when 0.373 moles of COCI2(g) are introduced into a 1.00 L vessel at 600 K. [COCI2] = [CO] M [Cl2] M ΣΣΣ

Write the Ke and Kp expressions for the following homogeneous equilibrium reactions: a) CO(g) + -O2(g) = CO2(g) b) 2CO,(g) = O,(g) + 2CO(g) c) N,0(g) = N2(g) + -0,(g)

Bromine monochloride is synthesized using the reaction Br₂ (g) + Cl₂(g) = 2 BrCl(g) Kp = 1.1 x 10-4 at 150 K A 208.0 L flask initially contains 0.953 kg of Br₂ and 1.184 kg of Cl₂. Calculate the mass of BrCl, 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: 6.D g %

Phosphorus trichloride gas and chlorine gas react to form phosphorus pentachloride gas. PCl3(g) + Cl2(g)  PCl5(g). A gas vessel is charged with a mixture of PCl3(g) and Cl2(g), which is allowed to equilibriate at 450 K. At equilibrium the partial pressures of the three gases are PPCl3 = 0.128 atm, PCl2 = 0.141 atm, and PPCl5 = 1.21 atm. (a) What is the value of Kp at this temperature? ______ (b) Does the equilibrium favor reactants or products? The equilibrium favors products. The equilibrium favors reactants.     Neither reactants nor products are favored.

Hh.53.

Consider the following reaction where K, = 6.50x10-3 at 298 K. 2NOBR(g) =2NO(g) + Br2(g) A reaction mixture was found to contain 8.79x10-2 moles of NOBR(g), 2.03x10-2 moles of NO(g), and 4.53x10 2 moles of Bro(g), in a 1.00 liter container. Is the reaction at equilibrium? If not, what direction must it run in order to reach equilibrium? The reaction quotient, Qc, equals The reaction A. must run in the forward direction to reach equilibrium. B. must run in the reverse direction to reach equilibrium. C. is at equilibrium.

Give Detailed Solution

For the reaction: H2 (g)+ Br2 (g)= 2 HBr(g) 104 Кр — 3.5 х 1495 K. at What is the value of Kp for each of the following reactions at 1495 K? (a) 2 HBr(g) - H2 (g)+ Br2 (g) Кр (b) H2 (g) + Br2 (g) = HBr(g) K, (c) HBr(g) = H2 (g) + Br2 (g) Kp =