016 32points 1 bar 0986923267 atm consider the

Info icon This preview shows pages 5–8. Sign up to view the full content.

View Full Document Right Arrow Icon
016 3.2points 1 bar = 0.986923267 atm Consider the reaction CuSO 4 (s) CuO(s) + SO 3 (g) . If Δ G = - 14 . 6 kJ at 950 C for this reac- tion, calculate Δ G for an SO 3 (g) pressure of 20 bar at this temperature. 1. - 14 . 6 kJ 2. 45.1 kJ 3. 15.9 kJ correct 4. - 45 . 1 kJ 5. 30.5 kJ Explanation: 017 3.2points Consider the reaction Ni(s) + 4 CO(g) Ni(CO) 4 (g) at a certain temperature. Calculate K for this reaction if, at equilibrium, the partial pressures of CO(g) and Ni(CO) 4 (g) are 1.25 atm and 6.65 atm over 1.00 kg of nickel. 1. 1.75 2. 2.2 3. 2.72 correct 4. 1.02 5. 3.4 Explanation: 018 3.2points At 990 C, K c is 1.6 for the reaction CO 2 (g) + H 2 (g) H 2 O(g) + CO(g) If 4.0 mol of CO, 3.0 mol of H 2 O, 2.0 mol of H 2 , and 1.0 mol of CO 2 are placed in a 5.0 liter container and allowed to reach equilibrium at 990 C, which response includes all of the following statements that are correct, and no others? I) The concentration of H 2 will be greater than 0.40 mol/L. II) The concentration of H 2 O will be less than 0.60 mol/L. III) The concentration of CO will be less than 0.80 mol/L.
Image of page 5

Info icon This preview has intentionally blurred sections. Sign up to view the full version.

View Full Document Right Arrow Icon
Version 324 – EXAM 2 – holcombe – (51395) 6 IV) The concentration of CO 2 will be greater than 0.20 mol/L. 1. I, II, III, and IV correct 2. I, II, and IV only 3. III only 4. I and II only 5. I and IV only Explanation: [H 2 O] ini = 3 . 0 mol 5 . 0 L = 0 . 6 M [CO] ini = 4 . 0 mol 5 . 0 L = 0 . 8 M [CO 2 ] ini = 1 . 0 mol 5 . 0 L = 0 . 2 M [H 2 ] ini = 2 . 0 mol 5 . 0 L = 0 . 4 M Q = [H 2 O] [CO] [CO 2 ] [H 2 ] = (0 . 6 M) (0 . 8 M) (0 . 2 M) (0 . 4 M) = 6 > K c = 1 . 6 Therefore equilibrium will shift to the left, in- creasing [CO 2 ] and [H 2 ] and decreasing [H 2 O] and [CO]. 019 3.2points The value of Q for a given reaction is a con- stant. 1. True 2. False correct Explanation: 020 3.2points The equilibrium constant for the gaseous re- action CO + H 2 O CO 2 + H 2 is 4.0 at a certain temperature. A reaction is carried out at this temperature starting with 2.0 mol/L of CO and 2.0 mol/L of H 2 O. What will be the equilibrium concentration of H 2 ? 1. 1.33 M correct 2. 0.75 M 3. 2.0 M 4. 1.5 M 5. 0.67 M Explanation: K = 4 . 0 [CO] ini = 2 . 0 mol / L [H 2 O] ini = 2 . 0 mol / L CO + H 2 O CO 2 + H 2 Ini, M 2 2 - - Δ, M - x - x + x + x Final, M 2 - x 2 - x x x Subsitute the final concentrations into the equation for K : K = [CO 2 ] [H 2 ] [CO] [H 2 O] 4 = ( x ) ( x ) (2 - x ) (2 - x ) Taking the square root of both sides gives 2 = ( x ) (2 - x ) 4 - 2 x = x 4 = 3 x x = 1 . 33 021 3.2points For the reaction CO(g) + 2 H 2 (g) CH 3 OH(g) Δ G rxn = 21 . 1 kJ/mol at 225 C. If you have a mixture with a P CO = 0 . 1 atm, P H 2 = 0 . 1 atm, and P CH 3 OH = 1 atm in a container at 225 C, 1. the reaction will move toward the prod- ucts to reach equilibrium.
Image of page 6
Version 324 – EXAM 2 – holcombe – (51395) 7 2. the reaction is at equilibrium. 3. the reaction will move toward the reac- tants to reach equilibrium. correct 4. the mixture can never achieve equilib- rium. Explanation: Δ G rxn > 0, so K < 1 and Q = 1000. Q > K , so the reaction will shift toward the reactants to reach equilibrium. 022 3.2points For the reaction A(aq) + B(aq) ←→ AB(aq) adding more A would change: 1. Standard change in free energy (Δ G o ) 2. only K 3. Reversibility of the reaction 4. only Q correct 5. Both K and Q Explanation: Adding more A would increase [A], and thus change the Q = [AB] / ([A][B]) for the reaction.
Image of page 7

Info icon This preview has intentionally blurred sections. Sign up to view the full version.

View Full Document Right Arrow Icon
Image of page 8
This is the end of the preview. Sign up to access the rest of the document.

{[ snackBarMessage ]}

What students are saying

  • Left Quote Icon

    As a current student on this bumpy collegiate pathway, I stumbled upon Course Hero, where I can find study resources for nearly all my courses, get online help from tutors 24/7, and even share my old projects, papers, and lecture notes with other students.

    Student Picture

    Kiran Temple University Fox School of Business ‘17, Course Hero Intern

  • Left Quote Icon

    I cannot even describe how much Course Hero helped me this summer. It’s truly become something I can always rely on and help me. In the end, I was not only able to survive summer classes, but I was able to thrive thanks to Course Hero.

    Student Picture

    Dana University of Pennsylvania ‘17, Course Hero Intern

  • Left Quote Icon

    The ability to access any university’s resources through Course Hero proved invaluable in my case. I was behind on Tulane coursework and actually used UCLA’s materials to help me move forward and get everything together on time.

    Student Picture

    Jill Tulane University ‘16, Course Hero Intern