Practice ProblemATTEMPT
For each change indicated, determine whether the equilibrium:
will shift to the right, shift to the left, or neither: (a) addition of
Want to see the full answer?
Check out a sample textbook solutionChapter 15 Solutions
Chemistry
- Question 21 Hydrogen iodide can be produced by the reversible reaction of hydrogen gas and iodine gas according to: H2(g) + I2(g) = 2HI(g) Keg for this reaction is 2.25 × 10³ at a temperature of 753°C. Calculate the concentration of HI in an equilibrium mixture if the concentration of H2 is 0.15 M and the concentration of I2 is 0.25 M. (a) 2.4 moles of H2(g) and 1.5 moles of I2(g) were placed in a sealed 2.0 L vessel maintained at a temperature of 753°C. After 2 hours, the number of moles of each gas present were as follows. (b) Moles of H2(g) Moles of I2(g) Moles of HI(g) 1.7 0.8 1.4 Show by calculation whether the forward or reverse reaction must increase for the system to come to a state of dynamic equilibrium.arrow_forwarde) none of the above 25. If K = 0.124 for A2 + 2B = 2AB, what is the value of K, for the reaction 4AB 2A2 + 4B? a) 0.124 b) 0.248 c) 65.0 d) – 0.124 e) 4.03 f) none of the abovearrow_forwardSelect all that apply. For the following equilibrium system, which of the following changes will form more CaCO3? CO2(g) + Ca(OH)2(s) = CaCO3(s) + H2O(l) 0 ΔΗ =-113 kJ rxn Decrease temperature at constant pressure (no phase change). Increase volume at constant temperature. Increase partial pressure of CO2. Remove one-half of the initial CaCO3.arrow_forward
- Question 2 Consider the following reactions, with equilibrium contants as shown: (1) C(s) + 0,(g) co,(g), K, (2) 2Ca(s) + O,(g)=2CaO(s). K, (3) 2Ca(s) + 2C(s) + 30,(g) =2CaCO,(s), K, In terms of K1, K2 and K3 , the equilibrium constant for the reaction CaO (s) +CO,(g) CACO,(s) can be expressed as: O a. O b. (K,) 2 + (K, + (K c. Od. O e. ) ( f. + (K None of the above.arrow_forwardFor the equilibrium system N2044) # 2NO26) what is the equilibrium constant when [N2O4) is 1.5 x 10-3 M and [NO2] is 0.57 M? (B) 2.2 × 102 . (A) 3.8 × 10² (C) 4.6 × 10-3 (D) 2.6 × 10-3arrow_forwardIncorrect Question 18 If 0.64 mol PCI, is placed in a 1.0 L flask and allowed to reach equilibrium at a given temperature, what is the final concentration of Cl₂ in the flask PCI5(g) --> PCl3(aq) + Cl2(g) Ke= 0.47 0.31 M 0.55 M 0.20 M 0.36 M C 0.96 Marrow_forward
- Practice Exercise At 1280°C the equilibrium constant (K) for the reaction Br2(g) 2Br(g) is 1.1 x 10 . If the initial concentrations are [Br2] 102 M, calculate the concentrations of these species at equilibrium. 6.3 x 10 2 M and [Br] = 1.2 X !!arrow_forwardWhich of the following statements is true regarding chemical equilibrium? Question 4 options: A) When equilibrium has been reached, all chemical reactions have ceased. B) When equilibrium has been reached, the rates of the forward and reverse reactions are equal. C) When equilibrium has been reached, the rate constants of the forward and reverse reactions are equal. D) When equilibrium has been reached, the value of the equlibrium constant is 1. E) When equilibrium has been reached, the limiting reagent has been consumed.arrow_forwardPractice Exercise At 1280°C the equilibrium constant (K.) for the reaction Br2(g) = 2Br(g) is 1.1 x 10-3. If the initial concentrations are [Br2] 6.3 x 10-2 M and [Br] = 1.2 × 10-2 M, calculate the concentrations of these species at equilibrium.arrow_forward
- Check Your Understanding In each of the following, determine the direction in which the equilibrium will shift in response to the indicated stress. (a) N2 (g) + 3 H2 (g) 2 2 NH3 (g); pressure is decreased Answer + Shift toward reactants (b) CO2(g)+ H2 (g) 2 CO(g) +H2O(g); pressure is increased Answer no changearrow_forwardQUESTION 18 Dinitrogen tetroxide partially decomposes according to the following equilibrium: N204 (g) 2NO2 (g) A 1.000-L flask is filled with 0.73 mol of N204. At equilibrium, 0.31 mol of N2O4 remains. Determine the equilibrium constant K for this reaction. Express your answer in decimal notation to 2 decimal places.arrow_forwardSuppose a 500. mL flask is filled with 0.20 mol of Cl, and 1.5 mol of HCl. The following reaction becomes possible: 0/3 H,(g) +Cl, (g) ~ 2HC1(g) The equilibrium constant K for this reaction is 0.754 at the temperature of the flask. Calculate the equilibrium molarity of Cl,. Round your answer to two decimal places. OM Explanation Check O 2022 McGraw Hill LLC. All Rights Reserved. Terms of Use Privacy Cer D? ? 23 」國 ITO00 FEB tv MacBook Air DII DD 888 F9 F7 F8 F6arrow_forward
- ChemistryChemistryISBN:9781305957404Author:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCostePublisher:Cengage LearningChemistryChemistryISBN:9781259911156Author:Raymond Chang Dr., Jason Overby ProfessorPublisher:McGraw-Hill EducationPrinciples of Instrumental AnalysisChemistryISBN:9781305577213Author:Douglas A. Skoog, F. James Holler, Stanley R. CrouchPublisher:Cengage Learning
- Organic ChemistryChemistryISBN:9780078021558Author:Janice Gorzynski Smith Dr.Publisher:McGraw-Hill EducationChemistry: Principles and ReactionsChemistryISBN:9781305079373Author:William L. Masterton, Cecile N. HurleyPublisher:Cengage LearningElementary Principles of Chemical Processes, Bind...ChemistryISBN:9781118431221Author:Richard M. Felder, Ronald W. Rousseau, Lisa G. BullardPublisher:WILEY