Calcium chloride 6-hydrate, CaC12.6H2O, dehydrates according to the equation
What is the pressure of water vapor at equilibrium with a mixture of
Want to see the full answer?
Check out a sample textbook solutionChapter 13 Solutions
Chemistry Atoms First2e
- Dinitrogen tetroxide, N2O4, is a colorless gas (boiling point, 21C), which dissociates to give nitrogen dioxide, NO2 a reddish brown gas. N2O4(g)2NO2(g) The equilibrium constant Kc at 25C is 0.125. What percentage of dinitrogen tetroxidc is dissociated when 0.0400 mol N2O4 is placed in a 1.00-L flask at 25C?arrow_forwardFluorine, F2, dissociates into atoms on heating. 12F2(g)F(g) The value of Kp at 842C is 7.55 102 What is the value of Kc at this temperature?arrow_forwardThe reaction 2 NO2(g) N2O4(g) has an equilibrium constant, Kc, of 170 at 25 C. If 2.0 103 mol of NO2 is present in a 10.-L. Flask along with 1.5 103 mol of N2O4, is the system at equilibrium? If it is not at equilibrium, does the concentration of NO2 increase or decrease as the system proceeds to equilibrium?arrow_forward
- Cyclohexane, C6H12, a hydrocarbon, can isomerize or change into methylcyclopentane, a compound of the same formula (C5H9CH3) but with a different molecular structure. sssss The equilibrium constant has been estimated to be 0.12 at 25 C. If you had originally placed 0.045 mol of cyclohexane in a 2.8-L flask, what would be the concentrations of cyclohexane and methylcyclopentane when equilibrium is established?arrow_forwardCalcium carbonate, CaCO3, decomposes when heated to give calcium oxide. CaO, and carbon dioxide, CO2. CaCO3(s)CaO(s)+CO2(g) Kp for this reaction at 900C is 1.040 What would be the yield of carbon dioxide (in grams) when 1.000 g of CaCO3 and 1.000 g CaO are heated to 900C in a 1.000-L vessel. (Ignore the volume occupied by the solids.) What would be the effect of adding a similar quantity of carbon dioxide to this equilibrium mixture? What would happen if the quantity of calcium carbonate were doubled?arrow_forwardSulfuryl chloride is used in organic chemistry as a chlorinating agent. At moderately high temperatures it decomposes as follows: SO2Cl2(g)SO2(g)+Cl2(g) with Kc = 0.045 at 650 K. a A sample of 8.25 g of SO2Cl2 is placed in a 1.00-L reaction vessel and heated to 650 K. What are the equilibrium concentrations of all of the species? b What fraction of SO2Cl2 has decomposed? c If 5 g of chlorine is inserted into the reaction vessel, what qualitative effect would this have on the fraction of SO2Cl2 that has decomposed?arrow_forward
- Antimony(V) chloride. SbCl5, decomposes on heating to give antimony(III) chloride, SbCl3, and chlorine. SbCl5(g)SbCl3(g)+Cl2(g) A closed 3.50-L vessel initially contains 0.0125 mol SbCl5. What is the total pressure at 248C when equilibrium is achieved? The value of Kc at 248C is 2.50 102.arrow_forwardAn experimenter places the following concentrations of gases in a closed container: [NOBr] = 7.13 102 M, [NO] = 1.58 102 M. [Br2] = 1.29 102 M. These gases then react: 2NOBr(g)2NO(g)+Br2(g) At the temperature of the reaction, the equilibrium constant Kc is 3.07 104. Calculate the reaction quotient, Qc, from the initial concentrations and determine whether the concentration of NOBr increases or decreases as the reaction approaches equilibrium. a Qc = 6.33 104; the concentration of NOBr decreases b Qc = 6.33 104; the concentration of NOBr increases c Qc = 1.58 104; the concentration of NOBr increases d Qc = 4.65 104; the concentration of NOBr decreases e Qc = 4.65 104; the concentration of NOBr increasesarrow_forwardThe following reaction has an equilibrium constant Kc equal to 3.59 at 900C. CH4(g)+2H2S(g)CS2(g)+4H2(g) For each of the following compositions, decide whether the reaction mixture is at equilibrium. If it is not, decide which direction the reaction should go. a [CH4] = 1.26 M, [H2S] = 1.32 M, [CS2] = 1.43 M, [H2] = 1.12 M b [CH4] = 1.25 M, [H2S] = 1.52 M, [CS2] = 1.15 M, [H2] = 1.73 M c [CH4] = 1.30 M, [H2S] = 1.41 M, [CS2] = 1.10 M, [H2] = 1.20 M d [CH4] = 1.56 M, [H2S] = 1.43 M, [CS2] = 1.23 M, [H2] = 1.91 Marrow_forward
- For the reaction N2(g)+3H2(g)2NH3(g) show that Kc = Kp(RT)2 Do not use the formula Kp = Kc(RT)5n given in the text. Start from the fact that Pi = [i]RT, where Pi is the partial pressure of substance i and [i] is its molar concentration. Substitute into Kc.arrow_forwardThe equilibrium constant Kc, for the reaction 2 NOCI(g) 2 NO(g) + Cl2(g) is 3.9 103 at 300 C. A mixture contains the gases at the following concentrations: [NOCl] = 5.0 103 mol/L, [NO] = 2.5 103 mol/L, and [Cl2] = 2.0 103 mol/L. Is the reaction at equilibrium at 300 C? If not, in which direction does the reaction proceed to come to equilibrium?arrow_forwardSuppose sulfur dioxide reacts with oxygen at 25C. 2SO2(g)+O2(g)2SO3(g) The equilibrium constant Kc equals 8.0 1035 at this temperature From the magnitude of Kc, do you think this reaction occurs to any great extent when equilibrium is reached at room temperature? If an equilibrium mixture is 1.0 M SO3 and has equal concentrations of SO2 and O2, what is the concentration of SO2 in the mixture? Does this result agree with what you expect from the magnitude of Kc?arrow_forward
- General 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 LearningChemistry & Chemical ReactivityChemistryISBN:9781337399074Author:John C. Kotz, Paul M. Treichel, John Townsend, David TreichelPublisher:Cengage LearningChemistry & Chemical ReactivityChemistryISBN:9781133949640Author:John C. Kotz, Paul M. Treichel, John Townsend, David TreichelPublisher:Cengage Learning
- Chemistry: The Molecular ScienceChemistryISBN:9781285199047Author:John W. Moore, Conrad L. StanitskiPublisher:Cengage LearningChemistryChemistryISBN:9781305957404Author:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCostePublisher:Cengage Learning