![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](http://img.homeworklib.com/questions/d8b63970-9afd-11eb-9c07-cbc866ce11df.png?x-oss-process=image/resize,w_560)
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16. Initially we place 0.24 mol of N204(g) in a 3.0 liter container. The following reaction...
1.00 mol of pure NO2 in a 40.0 liter container and we allowed it to react...
1.00 mol of pure NO2 in a 40.0 liter container and we allowed it to react per the reaction listed below at 150°C. At equilibrium, the concetration of NO in the container is found to be 0.0015 M. Use that information to calucalte the equilibrium constant for the following reaction. 2NO2 (g) ? 2NO (g) = O2 (g)
5. The equilibrium constant K for the dissociation of N204(g) to NO2(g) is 1700 at 500 K. If AH is 56.8 kJ/mol for this...
5. The equilibrium constant K for the dissociation of N204(g) to NO2(g) is 1700 at 500 K. If AH is 56.8 kJ/mol for this reaction, what will be the value of K at 300 K? (a) 132x106 (b) 1.11 x 104 (c) 0.188 (d) 15.5 (e) .54 x 107
5. The equilibrium constant K for the dissociation of N204(g) to NO2(g) is 1700 at 500 K. If AH is 56.8 kJ/mol for this reaction, what will be the value of...
Click Submit to complete this assessment. Question 4 Consider the reaction 2N02= N204 Initially, 0.401 mol...
Click Submit to complete this assessment. Question 4 Consider the reaction 2N02= N204 Initially, 0.401 mol NO2 is placed in an empty 1.0-L flask. At equilibrium, the concentration of N204 is 0.184 mol/L. Calculate Kc for the reaction. none of these 0 1.7x 10² 5.6 1.1 15 X 102 59 x 10-3 3,9
16. Consider the reaction: 2NO2(g) = N204(g) 4,Hº = -58.04 kJ/mol. Which of the following prediction...
16. Consider the reaction: 2NO2(g) = N204(g) 4,Hº = -58.04 kJ/mol. Which of the following prediction about the color change of system is CORRECT knowing that NO2 is brown and N204 is colorless (assuming all other side reactions can be neglected)? A. If the system at equilibrium is heated up, the color of the gas fades away. B. When the total pressure of the system at equilibrium is increased, the color of the gas deepens. C. If a colorless inert...
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....
16. Consider the equilibrium, 2HBr(9) H,(g)+Br (g). If 2.0 M HBr(g) is placed in a container,...
16. Consider the equilibrium, 2HBr(9) H,(g)+Br (g). If 2.0 M HBr(g) is placed in a container, then at equilibrium, the HBr(g) concentration is 1.4 M. Therefore, the equilibrium constant, Kc, for this reaction is approximately: (A) 0.046 (B) 0.064 (C) 0.21 (D) 0.26 07. For the reaction, N,O,(9) >2NO2(g), Ko = 0.40 at a certain temperature in an equilibrium mixture of the two gases, the concentration of N204 is 0.50 M. The concentration of NO2 in this mixture is approximately:...
The reaction N2O4(g) ⇌ 2NO2(g) has ∆G° = 13.3 kJ/mol at 25 °C. What is the...
The reaction N2O4(g) ⇌ 2NO2(g) has ∆G° = 13.3 kJ/mol at 25 °C. What is the value of ∆G, in kJ/mol, for this reaction at this temperature when [N2O4] = 3.0 M and [NO2] = 0.0010 M? Enter your answer to the tenths place. Do not include units. Include the sign if appropriate! Thank you for your help!
6. If 0.54 mol of H2S is placed in a 3.0 L container, what is the...
6. If 0.54 mol of H2S is placed in a 3.0 L container, what is
the equilibrium concentration of H2 at 710 C?
6. In the decomposition of hydrogen sulfide: 2H2S(9) + 2H2(g) + S2(g) K = 9.90 x 10-8 at 710°C If 0.54 mol H2S is placed in a 3.0 liter container, what is the equilibrium concentration of H2(g) at 710 °C? Can the small x approximation be used here? Justify it (see p. 768 of text). (1.9 x...
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.
please help!!!! For the following reaction 2NO2(g) = N204(9) AH° = -58.02 kJ/mol and AS° =...
please help!!!!
For the following reaction 2NO2(g) = N204(9) AH° = -58.02 kJ/mol and AS° = -176.6 J/mol K. What is AG for the reaction at 45.0°C when P_NO2 = P_N204 = 0.200 atm? Assume AH° and ASº are temperature independent. ple For the electrochemical cell 2 Al(s) + 3 Mn2+(aq) + 2 Al3+ (aq) + 3 Mn(s) (E° = 0.48 V, [A13+] = 1.0 M), what is the value of E when [ Mn2+] = 0.016 M? Assume Tis...
5. The equilibrium constant K for the dissociation of N204(g) to NO2(g) is 1700 at 500 K. If AH is 56.8 kJ/mol for this reaction, what will be the value of K at 300 K? (a) 132x106 (b) 1.11 x 104 (c) 0.188 (d) 15.5 (e) .54 x 107
5. The equilibrium constant K for the dissociation of N204(g) to NO2(g) is 1700 at 500 K. If AH is 56.8 kJ/mol for this reaction, what will be the value of...
Click Submit to complete this assessment. Question 4 Consider the reaction 2N02= N204 Initially, 0.401 mol NO2 is placed in an empty 1.0-L flask. At equilibrium, the concentration of N204 is 0.184 mol/L. Calculate Kc for the reaction. none of these 0 1.7x 10² 5.6 1.1 15 X 102 59 x 10-3 3,9
16. Consider the reaction: 2NO2(g) = N204(g) 4,Hº = -58.04 kJ/mol. Which of the following prediction about the color change of system is CORRECT knowing that NO2 is brown and N204 is colorless (assuming all other side reactions can be neglected)? A. If the system at equilibrium is heated up, the color of the gas fades away. B. When the total pressure of the system at equilibrium is increased, the color of the gas deepens. C. If a colorless inert...
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....
16. Consider the equilibrium, 2HBr(9) H,(g)+Br (g). If 2.0 M HBr(g) is placed in a container, then at equilibrium, the HBr(g) concentration is 1.4 M. Therefore, the equilibrium constant, Kc, for this reaction is approximately: (A) 0.046 (B) 0.064 (C) 0.21 (D) 0.26 07. For the reaction, N,O,(9) >2NO2(g), Ko = 0.40 at a certain temperature in an equilibrium mixture of the two gases, the concentration of N204 is 0.50 M. The concentration of NO2 in this mixture is approximately:...
6. If 0.54 mol of H2S is placed in a 3.0 L container, what is
the equilibrium concentration of H2 at 710 C?
6. In the decomposition of hydrogen sulfide: 2H2S(9) + 2H2(g) + S2(g) K = 9.90 x 10-8 at 710°C If 0.54 mol H2S is placed in a 3.0 liter container, what is the equilibrium concentration of H2(g) at 710 °C? Can the small x approximation be used here? Justify it (see p. 768 of text). (1.9 x...
please help!!!!
For the following reaction 2NO2(g) = N204(9) AH° = -58.02 kJ/mol and AS° = -176.6 J/mol K. What is AG for the reaction at 45.0°C when P_NO2 = P_N204 = 0.200 atm? Assume AH° and ASº are temperature independent. ple For the electrochemical cell 2 Al(s) + 3 Mn2+(aq) + 2 Al3+ (aq) + 3 Mn(s) (E° = 0.48 V, [A13+] = 1.0 M), what is the value of E when [ Mn2+] = 0.016 M? Assume Tis...
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