5. Consider the equilibrium where Kc = 85.0 at 460°C. The following mixture was prepared in a reactor at 460 °C with the concentrations [SO2] = 0.0200 M; [NO2] = 0.0200 M; [NO] = 0.100 M; [SO3] = 0.100 M. What will the concentrations of the four gases be when equilibrium is reached? SO2 (g) + NO2 (g) NO (g) + SO3 (g); Kc = 85.0 T 0.02 O02 010.1 一× +x 十と

5. Consider the equilibrium where Kc = 85.0 at 460°C. The following mixture was prepared in a reactor at 460 °C with the concentrations [SO2] = 0.0200 M; [NO2] = 0.0200 M; [NO] = 0.100 M; [SO3] = 0.100 M. What will the concentrations of the four gases be when equilibrium is reached? SO2 (g) + NO2 (g) NO (g) + SO3 (g); Kc = 85.0 T 0.02 O02 010.1 一× +x 十と

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

Chapter1: Chemical Foundations

Section: Chapter Questions

Problem 1RQ: Define and explain the differences between the following terms. a. law and theory b. theory and...

See similar textbooks

Similar questions

1. The diagrams below represent the following reversible chemical reaction: H2(g) + 12 (g) =2 HI (g) At 448 °C, the equilibrium constant, K, for this reaction is 51 Initial Conditions: Temperature = 448 °C Volume of the container = 2.0 L 0 = 1 mole H2 (g) = 1 mole I2 (g) 00 00 .. 00 00 •. What is the initial molar concentration of hydrogen. [H:]? What is the initial molar concentration of iodide, [I2]? M This system will reach equilibrium when rate of the forward reaction is equal to the rate of the reverse reaction. Write the equilibrium constant expression, Kc, for this reaction: Calculate the equilibrium concentrations for H;(g), I (g) and HI (g) H2(g}_ + l2 (g) 2 HI (g) [H2] [L2] [HI Initial Change Equilibrium +2x -X-
Consider the methanol synthesis reaction represented below. CO (g) + 2 H2 (g) = CH3OH (g) The initial concentrations were: [CO ] = 1.75 M, [H2] = 1.00 M, and [CH3OH] = 0.65 M. %3D %3D If the equilibrium [CO] was found to be 1.60 M, calculate the equilibirium constant (K) for this reaction. Note: Reaction temperature was kept constant throughout the process. 44 2.0 1.0 62
7. Nitrogen dioxide NO₂ exists in equilibrium with its dimer N₂O4. The equilibrium constant for this reaction is 6.1 x 106. 2 NO₂ (g) ← → N₂O4 (8) 4 If the total concentration of [N₂O4] and [NO₂] in a power plant plume were 3000 ppm, what is the concentration of each species? Show all equations and unknowns.
Consider the following equilibrium reaction:H2(g) + I2(g) ↔ 2HI(g)If the following equilibrium concentrations are observed: [H2] = 4.10 x 10-1M, [I2] = 5.54 x 10-2M, [HI] = 3.50 x 10-2M; what is the equilibrium constant
Say that you mix Fe3+ and SCN- together so that after mixing, the concentration of Fe3+ (aq) equals 0.0015 M , and the concentration of SCN- (aq) equals 5.5 x 10-4 M. You measure the concentration of product, FeSCN2+, after equilibrium forms. It is 7.2 x 10-5 M. Calculate the value of the equilibrium constant, K, for the reaction. F e 3 + ( a q ) + S C N − ( a q ) ⟷ F e S C N 2 + ( a q ) K = ? Group of answer choices 0.011 9.52 x 10-3 87.3 105
3.) For the following equilibrium reaction2NO2(g) ↔N2O4(g) + Δlook in the Tro text to see what LeChatelier's principle states about gases. Assume that the reaction occurs in an enclosed movable piston. [Hint: remember that PV=nRT] a.) The pressure of the reaction is increased. b.) The volume of the reaction is decreased. c.) The volume of the reaction is increased.
Given the following equilibrium constants at 700K, 2 N2O(g) (double arrow) 2 N2 (g) + O2(g) K1 = 8.2 x 1033NO2(g) (double arrow) 1⁄2 N2(g) + O2(g) K2 = 2.44 x 108N2O4(g) (double arrow) 2 NO2(g) K3 = 4.6 x 10-3 determine the values of the equilibrium constants for the following reaction. Show your equation-buildingprocess and your calculations. 2 N2O4(g) (double arrow) 2 N2O(g) + 3 O2(g) K =
Consider the reaction: 2S (s) + 30₂ (9)2SO3(g) Write the equilibrium constant for this reaction in terms of the equilibrium constants, K₁ and K₂, for the reactions below: 3 80 For answers with both a subscript and a superscript, enter the subscript first. For example, enter K if the first equilibrium constant should be squared. K = E D S(s) + O2(g) → SO₂(g) K₁ SO₂(g) + 1/2O₂(g) SO3(9) K₂ 13 с Submit Answer $ 888 FA F4 R F Show Hint V Retry Entire Group 9 more group attempts remaining % 5 T Cengage Learning Cengage Technical Support F G 6 B MacBook Air FO Y H & 7 N F7 U J * 00 8 ➤11 FO I M ( 9 V K O < H дв ) O L F10 question. P command F11 A ; Previous { + alt #2 “ . ? option Save and Exit I 1 delete 1 ente re
Consider the following reaction. 2 NO(g) + O2(g) −→ 2 NO2(g) KP = 0.25 The following initial amounts were placed into a container. Molecule Initial Pressure (atm) NO 0.7 O2 0.5 NO2 0.08 What are the equilibrium pressures for each species in the reaction? PNO = PO2 = PNO2 = Hint: Use the Wolfram Alpha website to solve the cubic equation. https://www.wolframalpha.com Here are some examples. https://www.wolframalpha.com/examples/mathematics/algebra/
Consider the formation of hydrogen fluoride: H₂(g) + F₂(g) → 2HF(g) If a 2.0 L nickel reaction container filled with 0.0063 M H₂ is connected to a 3.5 L container filled with 0.033 M F₂. The equilibrium constant, Kp, is 7.8e14. Calculate the molar concentration of HF at equilibrium.
The equilibrium constant (Kp) is 0.11 at a particular temperature for the reaction: N204(9) = 2NO2(9) Given the following sets of initial conditions, what is the net change that must occur for the reaction to reach equilibrium? Does the reaction shift left to reach equilibrium, does the reaction shift right to reach equilibrium or is the reaction at equilibrium at these initial concentrations so no net change will occur? A. PNO, = 0.105 atm, PN,0, = 0.146 atm В. PNO, = 0.093 atm, PN,0, = 0.054 atm С. PNO, = 0.180 atm, PN,0, = 0.134 atm %3D D. PNO, = 0.088 atm, PN,0, = 0.07 atm Е. PNO, = 0.055 atm, PN,0, = 0.06 atm %3D %D A. right B. left C. left D. equilibrium left right E. > >
Chapter 16 (Due 06/10, 23:00) O Saved 3 attempts left Check my work Be sure to answer all parts. Consider the following equilibrium process at 686°C: So CO;(g) + H2(g) = CO(g)+ H2O(g) Guidec The equilibrium concentrations of the reacting species are [CO] = 0.0500 M, [H2] = 0.0420 M, [CO2] = 0.0900 M, and [H,O] = 0.0350 M. ok (a) Calculate K, for the reaction at 686°C. int (b) If we add CO, to increase its concentration to 0.480 mol / L, what will the concentrations of all the gases be when equilibrium is reestablished? ences CO2: M H,: M CO: M H,O: M МaсВook Pro Thank We @ #3 $ 4. 5. 8. CO 3. 2.