166666.6 .0012 3. SO2(g)+ O2(g) = SO:(g) for which K -2.5x102 Initially Pso2=1.5atm, Poz-1.2atm, Pso3=1.2atm 6...
K and Q explain the directioninwhich the reaction will proceed ineach case. 3) SO2(g)+O2(g) SO3(g) for which Kp=2.5x10^-2 initially Pso2=1.5atm, Po2=1.2atm,Pso3=1.2atm 4)N2(g)+3H2(g) 2NH3(g) for which Kc=2.3 initially [N2]=0.0071 M, [H2]=9.17x10^-3 M, [NH3]=1.83x10^-4M
Module 9 Homework K and Q. Explain the direction in which the reaction will pro 1. CH.COOH(aq) + H20 (1) = CH.COO (aq) + Initially: [CH.COOH]-0.16 M. [CH,COO)-0.0028 the reason will proceed in each case. CHCOO (aq) + H2O (aq) for which K. - 4.2x10 M, CH.COO)-0.0028 M, [H,O)-0.0048 M 2. CO(g)+2H:(g) = CH,OH(g) for which K, -0.0012 Initially: Pco-0.03atm, P=0.004atm, ProR0.08atm. 3. SO2(g)+ O2(g) + SO.(g) for which K -2.5x102 Initially Pso2=1.5atm, Poz-1.2atm, Pso3=1.2atm 4. N2(g) + 3H2(g) +...
ignore #5 i couldnt remove picture 5. N2(g)+3H2(g) + 2NH3(g) for which K,-1.2x10-3 PN2=0.08atm, PH2=0.08atm, PnH3=1.2atm QUESTION 3 Calculate the pH of a buffer solution that contains 1.5 M acetic acid (CH,COOH) and 0.3M sodium acetate (CH,COONa). (Ka 1.8x10 for acetic acid] 3.5 None of these 4.0 3.8 49 QUESTION 4 Click Save and Submit to save and submit. Click Save All Answers to save all answers.
14. In which of the following reactions will Kc = Ko? ooo 4 NH3(g) + 3 O2(g) = 2 N2(g) + 6 H2O(g) 2 SO3(g) + 2 NO(g) = 2 SO2(g) + 2 NO2(g) 4 N2(g) + 2 O2(g) = 4 N2O(g) 6 SO2(g) + 3 O2(g) = 6 SO3(g) None of the above reactions have Kc = Kp.
2 O3(g) 3 O2(g) 4. [O3]i 0.5 M, and [O2]eq = 0.5 M. What is the value of K? What is the value of K if [O3]i = [O2]i = 1.66 M, and at equilibrium [O2] 2.71 M? 5. 6. Initially [O2] = 0.0040 M, and at equilibrium [O2] = 0.0039 M. What is K? Part B: Using K 2 NO(g) N2(g) + O2(g) 7. Initially [NO] = 0.772 M. If K = 30.25, what is [NOJeq? 8. Initially [N2]...
10. A study of the system, 4 NH3(g) + 7 O2(g) 2 N2O4(q) + 6 H2O(g), was carried out. A system was prepared with (NH3) = [02] = 3.60 M as the only components initially. At equilibrium. [N204) is 0.60 M. Calculate the equilibrium concentration of O2. a, 3.00 M b. 2.40 M c. 1.50 M d. 2.10 M e. 3.30 M 11. For the reaction, 2 SO2(g) + O2(g) 2 SO.(a), at 450.0 K the equilibrium constant, Kc, has...
For which of the following reactions is AS° > 0. Choose all that apply. 2C2H6(g) + 702(g) + 4CO2(g) + 6H2O(g) ONH4HS(s) + NH3(g) + H2S(g) S(s,rhombic) + 2CO(g) → SO2(g) + 2C(s,graphite) N2(g) + 3H2(g) + 2NH3(g) 2H2O(g) + 2Cl2(g) + 4HCI(g) + O2(g) Submit Answer Retry Entire Group 6 more group attempts remaining
The reaction and equilibrium constant are provided. 2 SO2(g) + O2(g) 92 SO3(g) K = 5.8 x 103 Which direction will the reaction proceed if [502] = 0.015 M. [02] = 0.010 Mand (SO3) = 0.200 M? no shift shifts to make more product shifts to make more reactant
At 850 K, the equilibrium constant for the reaction 2 SO, (g) + O2(g) = 250(g) is Kc = 15. If the given concentrations of the three gases are mixed, predict in which direction the net reaction will proceed toward equilibrium. Left No net reaction Right Answer Bank [S02] = 0.20 M [02] = 0.60 M [SO3) = 0.60 M [SO2] = 0.21 M [02] = 0.10 M [SO3] = 0.60 M [SO2] = 0.80 M [02] = 0.50 M...
For which of the following rcions is K=K? so o.35 © a. 203@) 3 02(@ O b. 2 CO2(g) = 2 CO(g) + O2(2) C.C(s) + H2O(E) ==H2(g) - CO() O d. NH3(g) = 3/2 Hy(@)12 N39) O e. CH.{9) -2 0,(@=CO2(g) + 2 )