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Find the Kor K, values for each of the reactions. 6. SO.(g)+ O2(g) → SO(g) K-2.5x10...
PRIMAR Module 8 Homework o ression for each reaction. Equilibrium Expressions: Write the K. (or k...
PRIMAR Module 8 Homework o ression for each reaction. Equilibrium Expressions: Write the K. (or k 1. CO(g) = CO(g) + Of(g) 2. CH.(g)+ O2(g) + CO2(g)+ H2O(g) 3. CH,COOH(aq) + H2O(1) = CH,COO (aq) + H,O (aq) 4. NO(g) + H2(g) = NH3(g) + H2O(1) 5. ZnS(s) + O2(g) = ZnO(s) + SO2(E) Find the Kor K, values for each of the reactions. 6. SO.(g). O.(g) = SO(g) K-2.5x10 at 25°C 7. N(g)+H:(g) = NH:(g) K-.0288 at 45°C 8....
Consider the reaction: N2O4 (g) container. Suppose initially [N2O. (g)l- 0 and [NO (g)lo - 3.0...
Consider the reaction: N2O4 (g) container. Suppose initially [N2O. (g)l- 0 and [NO (g)lo - 3.0 M. Further suppose that at some temperature the reaction proceeds to equilibrium and [NO (g)l - 2.0 M, i.e. the equilibrium concentration of [NO.g)).-2.0 M. Sketch a reasonable plot of molar concentrations of each substance as a function of time showing the progress of reaction to reach equilibrium. (Make sure the axes are labeled! Make sure you show linear increments along each axis!!!). 8....
1. The pH of a .02 M solution of monoprotic acid is 6.20. Find the K_a...
1. The pH of a .02 M solution of monoprotic acid is 6.20. Find the K_a of the acid 2. If .08 moles of a monoprotic acid are dissolved in 2 L of aqueous solution, it is then found that 14% of the acid has dissociated at equilibrium. Calculate the K_a for this monoprotic acid. 3. Consider the reaction: N2O4 (g)⇌ 2 NO2(g) taking place in a sealed, fixed volume container. Suppose initially [N2O4 (g)] 0 = 0 and [NO2(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....
A reaction in smog formation is 03 (g) + NO(g) + O2(g) + NO2 (g) K...
A reaction in smog formation is 03 (g) + NO(g) + O2(g) + NO2 (g) K = 6.0 x 1034 If the initial concentrations are [03] - 1.0 x 10-6 M, [NO] = 1.0 x 10-5 M, [NO2) = 2.5 x 104 M, and [02] = 8.2 x 103 M, is the system at equilibrium? If not, in which direction does the reaction proceed. The system is at equilibrium System is not at equilibrium. It must shift right to reach...
Name: (print clearly) 12. (10 pts) At 25 °C, K. - 3.75 for the reaction SO2(g) + NO2(g) SO(g) + NO(g). Calculate th...
Name: (print clearly) 12. (10 pts) At 25 °C, K. - 3.75 for the reaction SO2(g) + NO2(g) SO(g) + NO(g). Calculate the concentrations of all species at equilibrium, when the initial concentrations are all 0.800 M and equilibrium established. 13. (10 pts) Calculate the pH of a 0.10 M NaNO2 solution (K. - 4.5 x 104 for HNO.).
At 850 K, the equilibrium constant for the reaction 2 SO, (g) + O2(g) = 250(g)...
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...
The equilibrium constant for the reaction: H2(g) + I2(g) <--> 2HI(g) is 54 at 700 K....
The equilibrium constant for the reaction: H2(g) + I2(g) <--> 2HI(g) is 54 at 700 K. A mixture of H2, I2 and HI, each at 0.020 M, was introduced into a container at 700 K. Which of the following is true? At equilibrium, [H2] = [I2] = [HI]. No net change occurs because the system is at equilibrium. The reaction proceeds to the left producing more H2(g) and I2(g). The reaction proceeds to the right producing more HI(g). At equilibrium,...
Be sure to answer all parts. A) Calculate Kp for the following equilibrium: 3 O2(g) ⇌...
Be sure to answer all parts. A) Calculate Kp for the following equilibrium: 3 O2(g) ⇌ 2 O3(g) Kc =1.8 × 10 −56 at 450 K __× 10__ B) Gaseous ammonia was introduced into a sealed container and heated to a certain temperature: 2 NH3(g) ⇌ N2(g) + 3 H2(g) At equilibrium, [NH3] = 0.0233 M, [N2] = 0.119 M, and [H2] = 0.369 M. Calculate Kc for the reaction at this temperature. Kc = __
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)...
PRIMAR Module 8 Homework o ression for each reaction. Equilibrium Expressions: Write the K. (or k 1. CO(g) = CO(g) + Of(g) 2. CH.(g)+ O2(g) + CO2(g)+ H2O(g) 3. CH,COOH(aq) + H2O(1) = CH,COO (aq) + H,O (aq) 4. NO(g) + H2(g) = NH3(g) + H2O(1) 5. ZnS(s) + O2(g) = ZnO(s) + SO2(E) Find the Kor K, values for each of the reactions. 6. SO.(g). O.(g) = SO(g) K-2.5x10 at 25°C 7. N(g)+H:(g) = NH:(g) K-.0288 at 45°C 8....
Consider the reaction: N2O4 (g) container. Suppose initially [N2O. (g)l- 0 and [NO (g)lo - 3.0 M. Further suppose that at some temperature the reaction proceeds to equilibrium and [NO (g)l - 2.0 M, i.e. the equilibrium concentration of [NO.g)).-2.0 M. Sketch a reasonable plot of molar concentrations of each substance as a function of time showing the progress of reaction to reach equilibrium. (Make sure the axes are labeled! Make sure you show linear increments along each axis!!!). 8....
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....
A reaction in smog formation is 03 (g) + NO(g) + O2(g) + NO2 (g) K = 6.0 x 1034 If the initial concentrations are [03] - 1.0 x 10-6 M, [NO] = 1.0 x 10-5 M, [NO2) = 2.5 x 104 M, and [02] = 8.2 x 103 M, is the system at equilibrium? If not, in which direction does the reaction proceed. The system is at equilibrium System is not at equilibrium. It must shift right to reach...
Name: (print clearly) 12. (10 pts) At 25 °C, K. - 3.75 for the reaction SO2(g) + NO2(g) SO(g) + NO(g). Calculate the concentrations of all species at equilibrium, when the initial concentrations are all 0.800 M and equilibrium established. 13. (10 pts) Calculate the pH of a 0.10 M NaNO2 solution (K. - 4.5 x 104 for HNO.).
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...
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)...
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