Homework Answers
Let us write the equilibrium constants (Question 1-5)
![1. Kp = Pco][Poz] 1. Kp = [P.coz] 2. Kp = [Pco-][PHyo] [PC2H6][P02] 3. Kc = [CH3C00][H3O+] [CH3COOH][H20] 4. Kp = [Proz][PH2]](http://img.homeworklib.com/questions/9f99a1c0-dd0c-11eb-961b-69d37dd503de.png?x-oss-process=image/resize,w_560)
Question 6&7
![Kp. Ko (RT) ON An no. of moles of product- no. of moles of 180acla (6) Kp. [psos] , Ke: 2.5x 10 [PSollo, T 25 c = 298.15K un](http://img.homeworklib.com/questions/9ff23b90-dd0c-11eb-b172-df12c1ed62c3.png?x-oss-process=image/resize,w_560)
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PRIMAR Module 8 Homework o ression for each reaction. Equilibrium Expressions: Write the K. (or k...
Find the Kor K, values for each of the reactions. 6. SO.(g)+ O2(g) → SO(g) K-2.5x10...
Find the Kor K, values for each of the reactions. 6. SO.(g)+ O2(g) → SO(g) K-2.5x10 at 25°C 7. N.(g)+ H2(g) = NH,(g) K-.0288 at 45°C 8. Consider the reaction: N,O. (g) 2 NO2(g) taking place in a sealed, fixed volume container. Suppose initially [N,0. (g)bo= 0 and [NO.(g)] = 3.0 M. Further suppose that at some temperature the reaction proceeds to equilibrium and [NO_(g), - 2.0 M. Sketch a reasonable plot of molar concentrations of each substance as a...
Module 9 Homework K and Q. Explain the direction in which the reaction will pro 1....
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) +...
1) Write equilibrium expressions (Kg and K) for each of the following unbalanced equations: CaSO,(s) CaO...
1) Write equilibrium expressions (Kg and K) for each of the following unbalanced equations: CaSO,(s) CaO s)+ SO2(8)+ 02(g CH,COO (aq) + H20 (aq) C H,COOH(aq) + H2O(I) 2) The reaction 2HBr(g) H2(g)+ Br2(g) has a Ke value of 1.05 at 25°C. If [HBr] = 0.177 M, [H] 0.223 M and [Br] =0.111 M, in which direction will the system shift?
2) Write the equilibrium constant expressions for each of the following reactions. (For gas-phase reactions, write...
2) Write the equilibrium constant expressions for each of the following reactions. (For gas-phase reactions, write the Ke expression.) a) 2 NO(g) + O2(g) = 2 NO2(g) b) 4 Ag(s) + O2(g) + 2 Ag2O(S) c) CaCO3(s) + CO2(aq) + H2O(l) = Ca2+(aq) + 2 HCO3(aq) 3) a) Write the K, expressions for reactions a and b in problem 2. b) If the value of K for reaction a in problem 2 is 2.8 x 1011 at 200°C, what is...
1. Write down the equilibrium constant expressions, Ke and K, for each of the following reactions:...
1. Write down the equilibrium constant expressions, Ke and K, for each of the following reactions: (a) H(g)Cl(g) 2 HCl(g) (b) 2 C(s)+O2(g) 2 CO(g Ag (aq)Cl(aq) (c) AgCl(s) (d) 2 O(g) 3 0:(g) 2. A 1.0 L evacuated flask was charged with 0.020 mol of N,O, and 0.060 mol of NO2 at 25.0 C. After equilibrium was reached the NO2 concentration was found to be 0.0140 M. What is the equilibrium constant Ke for the reaction? N2O4(g) 2 NO:(g)...
Module 10 Homework Refer to the table at the beginning of the section for K. and...
Module 10 Homework Refer to the table at the beginning of the section for K. and K. values. 77 x 10-M Ba(OH), solution? What is the 1. What is the H.O ion concentration pH? 2. Calculate the OH ion concentration of a 6.2 x 10' M HNO, solution. 3. Calculate the pH of an aqueous solution containing 6.02 x 10 H,O' ions per liter. 4. Calculate the pH of a 1.2 M HCN solution. K.-4.9 x 100 for HCN 5....
1. Write down the equilibrium constant expressions, K, and K for each of the following reactions:...
1. Write down the equilibrium constant expressions, K, and K for each of the following reactions: (a) H2(g)C(g) 2 HCl(g) (b) 2 C(s)+0(g) 2 COg Ag (aq)Cl(aq) (c) AgCl(s) (d) 2 0,(g) 30,(g) 2. A 1.0 L evacuated flask was charged with 0.020 mol of N,O and 0.060 mol of NO, at 25.0 C. After equilibrium was reached the NO2 concentration was found to be 0.0140 M. What is the equilibrium constant K, for the reaction? N,0,(g)2 NO(g) 3. Ammonium...
Worksheet 15a (Intro) Rates & Equilibrium 5. Write the equilibrium expressions K, for each of the...
Worksheet 15a (Intro) Rates & Equilibrium 5. Write the equilibrium expressions K, for each of the following reactions: a. Na(g) + O2(8) 2NO(g) e. PC1:(g) =PC13(1) + Cl () b. SiH.(g) + 2C1_(g) = Siclag) + 2H2(g) f. Xe(g) + 3F5(g)=XeF6Kg) c. C(s) + CO/g) = 2CO(g) g. Pb(NO:) (aq) + 2KI(aq) = Pbl (s) + 2KNO (aq) d. Fe(s) + CO(g) = Fe(s) -CO(8) h. 2NaCl(s) + 302(g) + 2NaClO(s)
More Equilibrium: Please write equilibrium expressions for the following reactions: 1. i. 2 SO2 (g) +...
More Equilibrium: Please write equilibrium expressions for the following reactions: 1. i. 2 SO2 (g) + O2 (g) 2 SO3 (g) il. NH4NOs (s) N2O (g) +2 H20 (g) i CaCO3 (s) + CaO (s) + CO2 (g) iv. HNO2 (aq) +H2O (I) HaO* (aq) + NO2 (aq) 2. Predict which way the equilibrium will shift for each of the following changes: CO (g) + H2 (g) C (s) H2O (g) + heat i. increase [H2O] ii. increase [C0] iii....
6 The decomposition of ozone in the upper atmosphere is catalyzed by NO. The overall reaction...
6 The decomposition of ozone in the upper atmosphere is catalyzed by NO. The overall reaction and rate law are: rate k[O][NO] Os(g)+O(g)+20;(g); Write a possible mechanism that is consistent with rate law and identify an intermediate in the reaction. 7. A possible mechanism for the iodide ion catalyzed decomposition of hydrogen peroxide in aqueous solution is: -slow H2O:(aq) +I(aq)H;O(1) + 0I°(aq) -fast H20:(aq) +Or(aq)H:O()) +02(g)+l'(aq) What is: iv) the catalyst? iv) the intermediate ii) the rate law i) the...
Find the Kor K, values for each of the reactions. 6. SO.(g)+ O2(g) → SO(g) K-2.5x10 at 25°C 7. N.(g)+ H2(g) = NH,(g) K-.0288 at 45°C 8. Consider the reaction: N,O. (g) 2 NO2(g) taking place in a sealed, fixed volume container. Suppose initially [N,0. (g)bo= 0 and [NO.(g)] = 3.0 M. Further suppose that at some temperature the reaction proceeds to equilibrium and [NO_(g), - 2.0 M. Sketch a reasonable plot of molar concentrations of each substance as a...
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) +...
1) Write equilibrium expressions (Kg and K) for each of the following unbalanced equations: CaSO,(s) CaO s)+ SO2(8)+ 02(g CH,COO (aq) + H20 (aq) C H,COOH(aq) + H2O(I) 2) The reaction 2HBr(g) H2(g)+ Br2(g) has a Ke value of 1.05 at 25°C. If [HBr] = 0.177 M, [H] 0.223 M and [Br] =0.111 M, in which direction will the system shift?
2) Write the equilibrium constant expressions for each of the following reactions. (For gas-phase reactions, write the Ke expression.) a) 2 NO(g) + O2(g) = 2 NO2(g) b) 4 Ag(s) + O2(g) + 2 Ag2O(S) c) CaCO3(s) + CO2(aq) + H2O(l) = Ca2+(aq) + 2 HCO3(aq) 3) a) Write the K, expressions for reactions a and b in problem 2. b) If the value of K for reaction a in problem 2 is 2.8 x 1011 at 200°C, what is...
1. Write down the equilibrium constant expressions, Ke and K, for each of the following reactions: (a) H(g)Cl(g) 2 HCl(g) (b) 2 C(s)+O2(g) 2 CO(g Ag (aq)Cl(aq) (c) AgCl(s) (d) 2 O(g) 3 0:(g) 2. A 1.0 L evacuated flask was charged with 0.020 mol of N,O, and 0.060 mol of NO2 at 25.0 C. After equilibrium was reached the NO2 concentration was found to be 0.0140 M. What is the equilibrium constant Ke for the reaction? N2O4(g) 2 NO:(g)...
Module 10 Homework Refer to the table at the beginning of the section for K. and K. values. 77 x 10-M Ba(OH), solution? What is the 1. What is the H.O ion concentration pH? 2. Calculate the OH ion concentration of a 6.2 x 10' M HNO, solution. 3. Calculate the pH of an aqueous solution containing 6.02 x 10 H,O' ions per liter. 4. Calculate the pH of a 1.2 M HCN solution. K.-4.9 x 100 for HCN 5....
1. Write down the equilibrium constant expressions, K, and K for each of the following reactions: (a) H2(g)C(g) 2 HCl(g) (b) 2 C(s)+0(g) 2 COg Ag (aq)Cl(aq) (c) AgCl(s) (d) 2 0,(g) 30,(g) 2. A 1.0 L evacuated flask was charged with 0.020 mol of N,O and 0.060 mol of NO, at 25.0 C. After equilibrium was reached the NO2 concentration was found to be 0.0140 M. What is the equilibrium constant K, for the reaction? N,0,(g)2 NO(g) 3. Ammonium...
Worksheet 15a (Intro) Rates & Equilibrium 5. Write the equilibrium expressions K, for each of the following reactions: a. Na(g) + O2(8) 2NO(g) e. PC1:(g) =PC13(1) + Cl () b. SiH.(g) + 2C1_(g) = Siclag) + 2H2(g) f. Xe(g) + 3F5(g)=XeF6Kg) c. C(s) + CO/g) = 2CO(g) g. Pb(NO:) (aq) + 2KI(aq) = Pbl (s) + 2KNO (aq) d. Fe(s) + CO(g) = Fe(s) -CO(8) h. 2NaCl(s) + 302(g) + 2NaClO(s)
More Equilibrium: Please write equilibrium expressions for the following reactions: 1. i. 2 SO2 (g) + O2 (g) 2 SO3 (g) il. NH4NOs (s) N2O (g) +2 H20 (g) i CaCO3 (s) + CaO (s) + CO2 (g) iv. HNO2 (aq) +H2O (I) HaO* (aq) + NO2 (aq) 2. Predict which way the equilibrium will shift for each of the following changes: CO (g) + H2 (g) C (s) H2O (g) + heat i. increase [H2O] ii. increase [C0] iii....
6 The decomposition of ozone in the upper atmosphere is catalyzed by NO. The overall reaction and rate law are: rate k[O][NO] Os(g)+O(g)+20;(g); Write a possible mechanism that is consistent with rate law and identify an intermediate in the reaction. 7. A possible mechanism for the iodide ion catalyzed decomposition of hydrogen peroxide in aqueous solution is: -slow H2O:(aq) +I(aq)H;O(1) + 0I°(aq) -fast H20:(aq) +Or(aq)H:O()) +02(g)+l'(aq) What is: iv) the catalyst? iv) the intermediate ii) the rate law i) the...
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