Practice Problem ATTEMPT
Write equilibrium expressions for each of the following reactions:
Want to see the full answer?
Check out a sample textbook solutionChapter 15 Solutions
Chemistry
- At a certain temperature, the value of the equilibrium constant, K, for the reaction represented below is 2.0 x 105. What is the value of K for the reverse reaction at the same temperature? H2(g) + Br2(g) = 2HBr(g) (A) -2.0 x 10-5 (B) 5.0 x 10-6 (C) 2.0 x 10-5 (D) 5.0 x 10-5arrow_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_forward4:47 Question 1 of 13 Consider the following diagrams which show the progress for the reaction A (blue) B (red). The equilibrium constant (K) for this reaction is 0.8. At which point does the reaction reach equilibrium? BEFORE AFTER A) B) A) see problem image Submit C) D) B) see problem image Tap here or pull up for additional resourcesarrow_forward
- QUESTION 32 ICE tables are used for calculating changes in concentration in an equilibrium system. I represents the initial concentration, C the change in concentration between the initial value and the equilibrium value, and E the final concentration at equilibrium. The equilibrium constant for the following system is 0.0075 at 373 K. 2 503(g) = 2 50₂(g) + O₂(g) The initial concentrations of SO3, SO₂, and O₂ are 3.0 M, 2.0 M, and 1.0 M. Complete the ICE table to show the changes and equilibrium concentrations using the values from the following list. Provide your answer below: I C E [SO3] [SO₂] [0₂]arrow_forwardQuestion 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_forwardK=4.9x10-3 for the reaction CO2(g)+H2(g)⇄ CO(g)+H2O(g). If [CO2]=0.00025 M, [H2]=0.0010 M, & [CO]=0.000015 M, what is the concentration at equilibrium of H2O? Answer 8.2x10-5M I got 1.84x10^-14? Can someone explain this to me please.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_forwardGiven a K value of 4.6 X 10-12, would you expect a nearly complete reaction at equilibrium? yes no insufficient informationarrow_forward(Incorrect) For the reaction 2A(g) + B(s) C() + 2D(g) at 700 °C, Kc = 0.00577. Calculate the number of moles of D present at equilibrium if a mixture of 6.03 moles of C and 6.03 moles of D is heated to 700 °C in a 7.61-L container. 0.0074 mol (Your answer) 0.430 mol (Correct answer) 5.60 mol 0.056 molarrow_forward
- issue 6Choose the equilibrium in which the products are favored by a drop in pressure and the reactants favored by a drop in temperature.a) N2(g) + 3 H2(g) ⇔ 2 NH3(g) + 92.3 kJb) H2(g) + I2(g) + 51.8 kJ ⇔ 2 HI(g)c) PCl3(g) + Cl2(g) ⇔ PCl5(g) ΔH = -84.2 kJd) 2 NO2(g) ⇔ 2 NO(g) + O2(g) ΔH = +54 kJarrow_forwardWhat is the relationship of 5 points equilibrium constants for the following two reactions? (1) 2 NO,(g) > N,0,(g); K, (2) N,0,(g) > 2 NO,(g) K2 (a) K,= 1/ K2 O Option 1arrow_forwardHere are equilibrium constants for several reactions. Which of them favor the formation of products, and which favor the formation of reactants? (a) 4.5 X 10-8 (b) 32 (c) 4.5 (d) 3.0 x 10-7 (e) 0.0032arrow_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