Interpretation: The pressure at which
Concept introduction: The equilibrium constant
The equilibrium constant depends upon temperature.
Law of mass action is applicable on the equilibrium reactions.
The Le Chatelier’s principle states that the addition of the reactants shifts the equilibrium to the right while the addition of product shifts the equilibrium to the left at constant temperature.
The dissociation of the species is denotes by the symbol
To determine: The pressure at which
Want to see the full answer?
Check out a sample textbook solutionChapter 12 Solutions
Chemistry: An Atoms First Approach
- A gaseous material XY(g) dissociates to some extent to produce X(g) and Y(g): XY(g)X(g)+Y(g) A 2.00-g sample of XY (molar mass = 165 g/mol) is placed in a container with a movable piston at 25C. The pressure is held constant at 0.967 atm. As XY begins to dissociate, the piston moves until 35.0 mole percent of the original XY has dissociated and then remains at a constant position. Assuming ideal behavior, calculate the density of the gas in the container after the piston has stopped moving, and determine the value of K for this reaction of 25C.arrow_forward. Suppose that for the reaction PCl5(g)PCl3(g)+Cl2(g)it is determined, at a particular temperature. that the equilibrium concentrations are [PCl5(g)]=0.0711M,[PCl3(g)]=0.0302M, and [Cl2(g)]=0.0491M. Calculate the value of K for he reaction at this temperature.arrow_forwardThe density of trifluoroacetic acid vapor was determined at 118.1 C and 468.5 torr, and found to be 2.784 g/L. Calculate KC for the association of the acid.arrow_forward
- . At high temperatures, elemental nitrogen and oxygen react with each other to form nitrogen monoxide. N2(g)+O2(g)2NO(g)Suppose the system is analyzed at a particular temperature, and the equilibrium concentrations arc found to be [N2]=0.041M. [O2]=0.0078M, and [NO]=4.710M. Calculate the value of K for the reaction.arrow_forwardA 2.500-mol sample of phosphorus pentachloride, PCl5, decomposes at 160C and 1.00 atm to give 0.338 mol of phosphorus trichloride, PCl3, at equilibrium. PCl5(g)PCl3(g)+Cl2(g) What is the composition of the final reaction mixture?arrow_forwardAt a certain temperature, the reaction Xe(g)+2F2(g)XeF4(g)gives a 50.0% yield of XeF4, starting with Xe(Pxe=0.20atm) and F2(PF2=0.40atm). Calculate K at this temperature. What must the initial pressure of F2 be to convert 75.0% of the xenon to XeF4?arrow_forward
- The atmosphere consists of about 80% N2 and 20% O2, yet there are many oxides of nitrogen that are stable and can be isolated in the laboratory. (a) Is the atmosphere at chemical equilibrium with respect to forming NO? (b) If not, why doesnt NO form? If so, how is it that NO can be made and kept in the laboratory for long periods?arrow_forwardAt 500C, k for the for the formation of ammonia from nitrogen and hydrogen gases is 1.5105. N2(g)+3H2(g)2NH3(g)Calculate the equilibrium partial pressure of hydrogen if the equilibrium partial pressures of ammonia and nitrogen are 0.015 atm and 1.2 atm, respectively.arrow_forwardThe following reaction is earned out at 500 K in a container equipped with a movable piston. A(g)+B(g)C(g);Kc=10(at500K) After the reaction has reached equilibrium, the container has the composition depicted here. Suppose the container volume is doubled. a How does the equilibrium composition shift? b How does the concentration of each of the reactants and the product change? (That is, does the concentration increase, decrease, or stay the same?)arrow_forward
- . Gaseous phosphorus pentachloride decomposes according to the reaction PCl5(g)PCl3(g)+Cl2(g)The equilibrium system was analyzed at a particular temperature, and the concentrations of the substances present were determined to be [PCl5]=1.1102M,[PCl3]=0.325M. and [Cl2]=3.9103M. Calculate the value of K for the reaction.arrow_forwardAt 2300 K the equilibrium constant for the formation of NO(g) is 1.7 103. N2(g) + O2(g) 2 NO(g) (a) Analysis shows that the concentrations of N2 and O2 are both 0.25 M, and that of NO is 0.0042 M under certain conditions. Is the system at equilibrium? (b) If the system is not at equilibrium, in which direction does the reaction proceed? (c) When the system is at equilibrium, what are the equilibrium concentrations?arrow_forwardThe following data were collected for a system at equilibrium at 140°C. Calculate the equilibrium constant for the reaction, 3 H2(g) + N2(g) 5=^ 2 NHt(g) at this temperature. [H2] = 0.10 mol L_1, [NJ = 1.1 mol L"1, [NHJ = 3.6 X 10"-mol L'1arrow_forward
- Chemistry: An Atoms First ApproachChemistryISBN:9781305079243Author:Steven S. Zumdahl, Susan A. ZumdahlPublisher:Cengage LearningChemistryChemistryISBN:9781305957404Author:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCostePublisher:Cengage Learning
- Introductory Chemistry: A FoundationChemistryISBN:9781337399425Author:Steven S. Zumdahl, Donald J. DeCostePublisher:Cengage LearningChemistry: Principles and ReactionsChemistryISBN:9781305079373Author:William L. Masterton, Cecile N. HurleyPublisher:Cengage LearningGeneral Chemistry - Standalone book (MindTap Cour...ChemistryISBN:9781305580343Author:Steven D. Gammon, Ebbing, Darrell Ebbing, Steven D., Darrell; Gammon, Darrell Ebbing; Steven D. Gammon, Darrell D.; Gammon, Ebbing; Steven D. Gammon; DarrellPublisher:Cengage Learning