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

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

Chemistry

10th Edition

ISBN:9781305957404

Author:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste

Publisher:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste

Chapter1: Chemical Foundations

Section: Chapter Questions

Problem 1RQ: Define and explain the differences between the following terms. a. law and theory b. theory and...

See similar textbooks

Similar questions

Consider the following reaction where K. = 6.30 at 723 K: 2 NH3 (g) = N2 (g) + 3 H2 (g) A reaction mixture was found to contain 7.67x104 moles of NH3 (g), 2.38×102 moles of N2 (g), and 4.58×10-2 moles of H2 (g), in a 1.00 liter container. Indicate True (I) or False (F) for each of the following: ] 1. In order to reach equilibrium NH3(g) must be produced . 2. In order to reach equilibrium K. must decrease . v 3. In order to reach equilibrium N, must be consumed . 4. Qe is greater than K. |5. The reaction is at equilibrium. No further reaction will occur.
What were the initial partial pressures of NO and Cl2? Nitric oxide reacts with chlorine gas according to the following reaction: 2 NO (g) + Cl2 (g) = 2 NOCI (g) Kp = 0.27 at 700 K A reaction mixture initially contains equal partial pressures of NO and Cl2. At equilibrium, the partial pressure of NOC1 was measured to be 110 torr. Enter your answers numerically separated by a comma. ΑΣφ ? PNO, Po, 295.6,295.6 t. II
For reactions in the gas phase, an equilibrium constant may be written in terms of molarity (Kc) or in terms of partial pressures (Kp).The value of Kc for the reaction shown below is equal to 2.9×10-4 at 298 K.2NOBr(g)-> 2NO(g)+Br2(g) What is the value for Kp at 298 K for the reaction represented by the equation shown below? The value for the gas constant, R, is 0.08206 L • atm/mol • K.NOBr(g)-> NO(g)+ 1/2Br2 (g)
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 =