10. For the reaction at equilibrium H2(g) + CO2(g) + H2O(g) + CO(g) Kc = 0.10 at 420°C Which statement is true? a Slightly more H2O and CO is present than H2 and CO2. b. Slightly more H2 and CO2 is present than H2O and CO. C . The reaction vessel contains mostly CO and H2O. d. The reaction vessel contains mostly CO2 and H2O.

10. For the reaction at equilibrium H2(g) + CO2(g) + H2O(g) + CO(g) Kc = 0.10 at 420°C Which statement is true? a Slightly more H2O and CO is present than H2 and CO2. b. Slightly more H2 and CO2 is present than H2O and CO. C . The reaction vessel contains mostly CO and H2O. d. The reaction vessel contains mostly CO2 and H2O.

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...

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4. The hypothetical reaction shown below has a Kc = 4.0 x 10° at 500 K. The equilibrium partial pressures for A2 and AB: are 2.0 atm and 1.3 atm, respectively. What is the equilibrium partial pressure of B2? * %D A2(g) +3 B2(g) 2 AB3(g) 0.71 atm O 0.09 atm 0.06 atm O 0.94 atm
68. Each reaction is allowed to come to equilibrium, and then the volume is changed as indicated. Predict the effect (shift right, shift left, or no effect) of the indicated volume change. a. CO(g) + H2O(g) = CO2(8) + H2(g) (volume is decreased) b. PC13(g) + Cl2(g) = PCI3(g) (volume is increased) c. CaCO3(s) = CaO(s) + CO2(g) (volume is increased)
The following reactions have been allowed to reach equilibrium. Consider the following changes that are introduced to the system and predict the direction of the equilibrium thift (to the left or to the nght). If no equilibrium shift is expected, write "no change". a. PCl (g)+Ch(g) PCl (g); some PCL is removed Ans. b. 2 SO (g) 2 SO:(g) + O:(g); pressure is increased Ans. c. COBR:(g)+ 18.2 kcal CO(g) + Bra:(g); temperature is increased Ans. d. 2 NOBr(g) 2 NO(g) + Br:(g); catalyst is added Ans. e. 2 NO(g) + Cl:(g)2 NOCI(g); exothemic; temperature is increased Ans. £ BACO (s) BaO(s) + CO:(g); Bao is added Ans. g PCl (g) + Cl(g) PCl-(g)+ energy; the reaction is cooled Ans. h. HPO, (aq) + H.O(I) PO, "(aq) + H.O (aq); NaOH is added Ans. i C:H. (g) +L(g) C:Hal: (g)+ heat; a catalyst is added Ans. j. AgBr (3) Ag (aq) +Br(aq); AgBr is added Ans.
At a particular temperature, KP = 0.25 for the reaction N2O4 (g) ⇌ 2NO2 (g) a. A flask containing only N2O4 at an initial pressure of 5 atm is allowed to reach equilibrium. Calculate the equilibrium partial pressures of the gases. b. A flask containing only NO2 at an initial pressure of 9.0 atm is allowed to reach equilibrium. Calculate the equilibrium partial pressures of the gases. c. From your answers to parts a and b, does it matter from which direction an equilibrium position is reached?
The decomposition of PCl5 occurs by the equilibrium process PCl5(g) = PCl3(g) + Cl2(g) DH, = 92.5 kJ mol–1 If the reaction is initially at equilibrium, explain what happens when the temperature is lowered. Select one: a. The equilibrium shifts left b. The concentration of Cl2(g) will increase c. No change d. The equilibrium shifts right
Which of the following equilibrium systems will shift to the right (toward the products) when pressure isincreased? A. 2 PbS(s) + 3 O2(g) ⇋ 2 PbO(s) + 2 SO2(g)B. PCl5(g) ⇋ PCl3(g) + Cl2(g)C. H2(g) + CO2(g) ⇋ H2O(g) + CO(g)D. All of these will shift to the right.E. None of these will shift to the right.
d. he following system establishes an equilibrium at 545 K: NH₂HS (s)- NH₂ (8) + H₂S (8) AND >O Briefly explain the effect in terms of the expected shift (toward reactant, toward product or no change) of each of the following: a b. The volume of the container is doubled. The temperature of the system is raised to 825 K C. Some additional solid NH4HS is added. The reaction flask has 1.25 atm of the inert gas argon added to it. 5. (10 points) At 355 K, a 10.00 L reaction flask is charged with 1.44 atm each of hydrogen and fluorine gas. The following reaction takes place: H2 (8) + F2 (g) = 2 HF (g) Kp = 176 Based on building an ICE table, determine the partial pressure of H2, F2 and HF once equilibrium has been established.
Consider the following reaction and its equilibrium constant: 12(g) 2 I(g) Kp = 0.209 A reaction mixture contains 0.89 atm 12 and 1.88 atm I. Which of the following statements is TRUE concerning this system? OA. The reaction quotient will decrease. OB. The reaction will shift in the direction of reactants. OC. The system is at equilibrium. D. The reaction will shift in the direction of products. OE. The equilibrium constant will decrease.
Consider the following system at equilibrium at 698 K: 2 HI (g)=H2 (g) + I2 (g) When some H2 (g) is added to the equilibrium system at constant temperature: The reaction must: A. Run in the forward direction to reestablish equilibrium. B. Run in the reverse direction to reestablish equilibrium. C. Remain the same. It is already at equilibrium. The concentration of I, will: A. Increase. B. Decrease. C. Remain the same. Submit Answer Retry Entire Group 9 more group attempts remaining
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3. Given the reaction: 2NH3(g) → N2(g) + 3H2(g)Determine the Kc of the reaction at 472°C if the equilibrium concentrations were determined to be[H2] = 0.1270 M[N2] = 0.04020 M[NH3] = 0.002720 M
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