Which of the following statements is correct about the addition of solid NH4Cl to NH3? a. The concentration of NH4 increases and those of NH3 and OH- decrease. b. The concentration of both NH4 and NH3 increase but tha of OH decreases. C. The concentrations of both NH4 and NH3 increase but that of NH3 decreases. d. The concentrations of all species in the equilibrium increase.

Which of the following statements is correct about the addition of solid NH4Cl to NH3? a. The concentration of NH4 increases and those of NH3 and OH- decrease. b. The concentration of both NH4 and NH3 increase but tha of OH decreases. C. The concentrations of both NH4 and NH3 increase but that of NH3 decreases. d. The concentrations of all species in the equilibrium increase.

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

Chapter13: Chemical Equilibrium

Section: Chapter Questions

Problem 23Q: Consider the reaction 2N2O(g) + O2(g) 4NO(g) Suppose the system is at equilibrium, and then an...

See similar textbooks

Similar questions

Consider the reaction 2N2O(g) + O2(g) 4NO(g) Suppose the system is at equilibrium, and then an additional mole of N2O(g) is injected into the system at constant temperature. Once the reaction reestablishes equilibrium, has the amount of N2O increased or decreased from its original equilibrium amount? Explain. What happens to the value of the equilibrium constant with this change?
12.102 A chemical engineer is working to optimize the production of acrylonitrile to be used in the manufacture of carbon fibers. The reaction being used is the combination of propene gas, ammonia, and oxygen. The reaction is normally carried out at moderately high temperatures so all species are in the gas phase. (a) Write the equilibrium constant expression for this reaction. (b) The boiling point of acrylonitrile is 77 °C, and that of propene is -48 °C. What would the equilibrium expression be if this reaction were carried out at room temperature? (c) What characteristic of this reaction might cause the engineer to desire carrying out this reaction at room temperature?
Consider a cylinder containing a mixture of liquid carbon dioxide in equilibrium with gaseous carbon dioxide at an initial pressure of 65 atm and a temperature of 20 C. Sketch a plot depicting the change in the cylinder pressure with time as gaseous carbon dioxide is released at constant temperature.
The conversion of oxygen to ozone has a very small equilibrium constant. 3/2 O2(g) O3(g) K = 2.5 1029 (a) What is the value of K when the equation is written using whole-number coefficients? 3 O2(g) 2 O3(g) (b) What is the value of K for the conversion of ozone to oxygen? 2 O3(g) 3 O2(g)
Ozone, O3, is an essential component in our atmosphere and very damaging to lungs when inhaled. It can be formed by the reaction of O2O2with OOaccording the reaction below. Reaction of interest: 1/2O2(g)+1/2O(g)⇄1/2O3(g). K=? Use the reactions below and the equilibrium constants provided to calculate the equilibrium constant for the production of ozone from O2and O Related reactions: NO2(g)⇄O(g)+NO(g)K=6.8•10−49 O3(g)+NO(g)⇄NO2(g)+O2(g)K=5.8•10−34
2 NH3 (g) ⟷ N2 (g) + 3 H2 (g) Kp = 0.83 If the initial pressures for all three species is 1 atm what is the equilibrium pressure of H2? (Hint: Your quadratic will have two solutions, which one is impossible?)
Hydrogen, a potential fuel, is found in great abundance in water. To separate the hydrogen from the oxygen, water must be thermally decomposed. At 1000°C, the equilibrium constant for this reaction is 7.3 x 10-182H2O(g) + heat <-> 2H2(g) + O2(g) a) If the initial concentration of H2O is 0.350 M, what is the equilibrium concentration of H2? b) Suggest three stresses that could be applied to the equilibrium system to produce more hydrogen.
Given the following data at a certain temperature,2N2(g) + O2(g) 2N2O(g) K1 = 1.2  10–35N2O4 (g) 2NO2 (g) K2 = 4.6  10–3½ N2(g) + O2 NO2 (g) K3 = 4.1  10–9Calculate the equilibrium constant for the following reaction:N2O (g) + O2(g) N2O4(g)
Write the balanced chemical equation for the reaction of the equilibrium between nitrogen dioxide and dinitrogen tetroxide. Calculate the equilibrium concentration of: NO2 if initially the concentration of NO2 is 0.750 M and N2O4 is 0.00 M. The value of K at this temperature is 1.15.
Calculate the equilibrium partial pressure of NO2 and N2O4.
Ammonia is produced by the Haber process, in which nitrogen and hydrogen are reacted directly using an iron mesh with oxides as a catalyst. For the reaction: N2(g) + 3H2(g) 2NH3(g) equilibrium constants (K values) as a function of temperature are: 300 Celsius, 4.34 x 10^-3 500 Celsius, 1.45 x 10^-5 600 Celsius, 2.25 x 10^-6 Is the reaction exothermic or endothermic? How did you determine this? How do I show that it is exothermic?
During the day, solar radiation is absorbed by NO3(g)NO3(g), resulting in its decomposition. Which of the following best explains whether the equilibrium concentration of N2O5(g)N2O5(g) in the atmosphere in the daytime is different from that in the nighttime, and why?