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Consider the reaction: N2O4 (g) container. Suppose initially [N2O. (g)l- 0 and [NO (g)lo - 3.0...
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...
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)]...
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....
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....
25. Suppose that 2.00 moles of N2O4 are initially injected into a 1.00 L reaction vessel...
25. Suppose that 2.00 moles of N2O4 are initially injected into a 1.00 L reaction vessel held at 100oC. Calculate the equilibrium concentrations. N2O4 (g) <-> 2NO2 (g) Kc= 0.20 Please show all work for thumbs up
Nitrogen dioxide dimerizes according to the following reaction: 2NO2(g)⇌N2O4(g) Kp=6.7at298K A 2.35-L container contains 0.057 mol...
Nitrogen dioxide dimerizes according to the following reaction: 2NO2(g)⇌N2O4(g) Kp=6.7at298K A 2.35-L container contains 0.057 mol of NO2 and 0.084 molof N2O4at298K. Calculate Kc for the reaction. Express the equilibrium constant with respect to concentration to three significant figures. Calculate Q for the reaction. Express the reaction quotient to three significant figures.
Nitrogen dioxide dimerizes according to the following reaction: 2NO2(g)⇌N2O4(g) Kp=6.7at298K A 2.35-L container contains 0.052 mol...
Nitrogen dioxide dimerizes according to the following reaction: 2NO2(g)⇌N2O4(g) Kp=6.7at298K A 2.35-L container contains 0.052 mol of NO2 and 0.087 mol of N2O4at298K. Calculate Q for the reaction.
Hydrogen iodide decomposes according to the reaction 2 HI(g) = H2(g) +1268) A sealed 1.50-L container...
Hydrogen iodide decomposes according to the reaction 2 HI(g) = H2(g) +1268) A sealed 1.50-L container initially holds 0.00623 mol of H2, 0.00414 mol of 12, and 0.0244 mol of HI at 703 K. When equilibrium is reached, the concentration of H2(g) is 0.00467 M. What are the concentrations of HI(g) and 12(g)? 112le [HI]
16. Initially we place 0.24 mol of N204(g) in a 3.0 liter container. The following reaction...
16. Initially we place 0.24 mol of N204(g) in a 3.0 liter container. The following reaction then occurred: N204(g)2NO2(g). If [NO2] 0.072 M, what is the value of K? a) 1.2 x 10-1 M d) 8.8 x 106 M b) 3.1x 104 M e) none of these c) 6.1 x 104 M
Suppose a 5.00 L nickel reaction container filled with 0.0090 M H2 is connected to a...
Suppose a 5.00 L nickel reaction container filled with 0.0090 M H2 is connected to a 3.00 L container filled with 0.201 M F2. Calculate the molar concentration of H2 at equilibrium.
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...
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....
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....
Hydrogen iodide decomposes according to the reaction 2 HI(g) = H2(g) +1268) A sealed 1.50-L container initially holds 0.00623 mol of H2, 0.00414 mol of 12, and 0.0244 mol of HI at 703 K. When equilibrium is reached, the concentration of H2(g) is 0.00467 M. What are the concentrations of HI(g) and 12(g)? 112le [HI]
16. Initially we place 0.24 mol of N204(g) in a 3.0 liter container. The following reaction then occurred: N204(g)2NO2(g). If [NO2] 0.072 M, what is the value of K? a) 1.2 x 10-1 M d) 8.8 x 106 M b) 3.1x 104 M e) none of these c) 6.1 x 104 M
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