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6 (13 pts) Given the system: 4NH3(g) + 302(g) = 2N2(g) + 6H2O(1) AH=-1530.4 kJ a)...
Given the system: 4NH3(g) + 302(g) = 2N2(g) + 6H2O(1) AH=-1530.4 kJ a) Discuss (and provide...
Given the system: 4NH3(g) + 302(g) = 2N2(g) + 6H2O(1) AH=-1530.4 kJ a) Discuss (and provide reasoning) how the ammonia (NH3) concentration will be affected at equilibrium: i) Removing O2: ii) Adding additional water: iii) Increasing volume:
AH = - 1132 kJ 5. Calculate AH for: 4NH3 + 302 → 2N2 + 6H2009...
AH = - 1132 kJ 5. Calculate AH for: 4NH3 + 302 → 2N2 + 6H2009 given the following reactions: (10 points) show all setup & work 2NH3 + 02@ → 2N02@ + 3H20W 3NO2® + 4NH3 + N2@ + 6H2000 AH = -2740 kJ
1. For the reaction 4NH3(g) + 302(g) → 2N2(g) + 6H2O(g) it was found that at...
1. For the reaction 4NH3(g) + 302(g) → 2N2(g) + 6H2O(g) it was found that at a given temperature and a certain time the rate of formation of N2(g) was 0.27 mol L's-1. a.) At what rate was water being formed? b.) At what rate was NH3 being consumed? c.) At what rate was O2 being consumed?
4. Consider the following system 2 N(g) + 6 HOU) AH- 1530.4 kJ (a) How will...
4. Consider the following system 2 N(g) + 6 HOU) AH- 1530.4 kJ (a) How will the amount of ammonia at equilibrium be affected by (I) removing O.(g)? ammon (a w、ll inrease (2) adding N:(g)? (3) adding water? (4) expanding the container at constant pressure? (5) increasing the temperature? (b) Which of the above factors will increase the value of K? Which will decrease it?
(a) For the reaction 2NO2 (g) 2NO (g) + 02 (g) K # 0.50. Predict the...
(a) For the reaction 2NO2 (g) 2NO (g) + 02 (g) K # 0.50. Predict the direction in which the system will move to reach equilibrium if the initial gas pressures are NO: 0.20 atm . NO2: 0.20 atm (answer: to the right because Q< K) .NO2: 0.0961 atm 02: 0.0589 atm NO: 0.280 atm (answer: the system is already at equilibrium because Q -K) O2: 0.20 atm NO: 0.56 atm NO2: 0.20 atm (answer: to the left because Q>...
Ammonia reacts with oxygen according to the equation: 4NH3(g) +502(g) → 4NO(g) + 6H2O(g) AH.,.. =...
Ammonia reacts with oxygen according to the equation: 4NH3(g) +502(g) → 4NO(g) + 6H2O(g) AH.,.. = 4906 kJ Calculate the heat (in kJ) associated with the complete reaction of 355 g of NH3. Express your answer with the appropriate units. Value Units
6. Consider the following equilibrium, 2N2(g) + 6H20(0) 4NH3(g) + 3O2(g) AH =-1531 kJ/mol a. Write...
6. Consider the following equilibrium, 2N2(g) + 6H20(0) 4NH3(g) + 3O2(g) AH =-1531 kJ/mol a. Write the equilibrium constant expression for K. and for Kp, if appropriate, for the reaction. b. State whether the equilibrium is heterogeneous or homogeneous. c. State how the equilibrium would respond to the addition of some of the water from the system. d. State how the equilibrium would respond to a decrease in the partial pressure of ammonia (NHa). e. State how the equilibrium would...
Question 8. A study of the system, 4NH3(g) + 7O2 ----------> 2N2O4(g) * 6H2O(g), was carried...
Question 8. A study of the system, 4NH3(g) + 7O2
----------> 2N2O4(g) * 6H2O(g), was carried out. A system was
prepared with [NH3]=[O2]= 3.60M as the only components intially. At
equilibrium, [N2O4] is 0.600M. Calculatevthe equilibrium
concentratiok of NH3.
AUIUS H2Se, HzTe, and H2S in order of increasing acid strength. 8. A study of the system, 4NH3(g) + 702(9) 2N2O4(9) + 6H2O(g), was carried out. A system was prepared with (NH2) = (O2) = 3.60 M as the only components...
Consider the following reaction: 4NH3(g) + 502(g) – 4NO(g) + 6H2O(g); AH = -906 kJ Now...
Consider the following reaction: 4NH3(g) + 502(g) – 4NO(g) + 6H2O(g); AH = -906 kJ Now answer the following two questions. 1. Which condition will release more heat? A. Combining 4.0 g of NH3 with excess O2 or B. Combining 5.0 g of O2 with excess NH3 2. How much heat will be released from your answer in question 1? Condition will release more heat and the value of this heat energy is
Consider the following system at equilibrium. N2(g) + 3 H2 (g) 2 NH3(g) + 92.24 kJ...
Consider the following system at equilibrium. N2(g) + 3 H2 (g) 2 NH3(g) + 92.24 kJ <--> Which response includes all of the following that will shift the equilibriu to the right, and no others? I. increasing the temperature III. increasing the pressure II. decreasing the temperature IV. decreasing the pressure VI. adding some NH3 V. removing some NH3 VII. removing some N2 VIII. adding some N2 a) I, IV, VI, and VII c) I, VI, and VII e) II,...
Given the system: 4NH3(g) + 302(g) = 2N2(g) + 6H2O(1) AH=-1530.4 kJ a) Discuss (and provide reasoning) how the ammonia (NH3) concentration will be affected at equilibrium: i) Removing O2: ii) Adding additional water: iii) Increasing volume:
AH = - 1132 kJ 5. Calculate AH for: 4NH3 + 302 → 2N2 + 6H2009 given the following reactions: (10 points) show all setup & work 2NH3 + 02@ → 2N02@ + 3H20W 3NO2® + 4NH3 + N2@ + 6H2000 AH = -2740 kJ
1. For the reaction 4NH3(g) + 302(g) → 2N2(g) + 6H2O(g) it was found that at a given temperature and a certain time the rate of formation of N2(g) was 0.27 mol L's-1. a.) At what rate was water being formed? b.) At what rate was NH3 being consumed? c.) At what rate was O2 being consumed?
4. Consider the following system 2 N(g) + 6 HOU) AH- 1530.4 kJ (a) How will the amount of ammonia at equilibrium be affected by (I) removing O.(g)? ammon (a w、ll inrease (2) adding N:(g)? (3) adding water? (4) expanding the container at constant pressure? (5) increasing the temperature? (b) Which of the above factors will increase the value of K? Which will decrease it?
(a) For the reaction 2NO2 (g) 2NO (g) + 02 (g) K # 0.50. Predict the direction in which the system will move to reach equilibrium if the initial gas pressures are NO: 0.20 atm . NO2: 0.20 atm (answer: to the right because Q< K) .NO2: 0.0961 atm 02: 0.0589 atm NO: 0.280 atm (answer: the system is already at equilibrium because Q -K) O2: 0.20 atm NO: 0.56 atm NO2: 0.20 atm (answer: to the left because Q>...
Ammonia reacts with oxygen according to the equation: 4NH3(g) +502(g) → 4NO(g) + 6H2O(g) AH.,.. = 4906 kJ Calculate the heat (in kJ) associated with the complete reaction of 355 g of NH3. Express your answer with the appropriate units. Value Units
6. Consider the following equilibrium, 2N2(g) + 6H20(0) 4NH3(g) + 3O2(g) AH =-1531 kJ/mol a. Write the equilibrium constant expression for K. and for Kp, if appropriate, for the reaction. b. State whether the equilibrium is heterogeneous or homogeneous. c. State how the equilibrium would respond to the addition of some of the water from the system. d. State how the equilibrium would respond to a decrease in the partial pressure of ammonia (NHa). e. State how the equilibrium would...
Question 8. A study of the system, 4NH3(g) + 7O2
----------> 2N2O4(g) * 6H2O(g), was carried out. A system was
prepared with [NH3]=[O2]= 3.60M as the only components intially. At
equilibrium, [N2O4] is 0.600M. Calculatevthe equilibrium
concentratiok of NH3.
AUIUS H2Se, HzTe, and H2S in order of increasing acid strength. 8. A study of the system, 4NH3(g) + 702(9) 2N2O4(9) + 6H2O(g), was carried out. A system was prepared with (NH2) = (O2) = 3.60 M as the only components...
Consider the following reaction: 4NH3(g) + 502(g) – 4NO(g) + 6H2O(g); AH = -906 kJ Now answer the following two questions. 1. Which condition will release more heat? A. Combining 4.0 g of NH3 with excess O2 or B. Combining 5.0 g of O2 with excess NH3 2. How much heat will be released from your answer in question 1? Condition will release more heat and the value of this heat energy is
Consider the following system at equilibrium. N2(g) + 3 H2 (g) 2 NH3(g) + 92.24 kJ <--> Which response includes all of the following that will shift the equilibriu to the right, and no others? I. increasing the temperature III. increasing the pressure II. decreasing the temperature IV. decreasing the pressure VI. adding some NH3 V. removing some NH3 VII. removing some N2 VIII. adding some N2 a) I, IV, VI, and VII c) I, VI, and VII e) II,...
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