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![2 NO + 02 - 2002 I 0.89 0.87 C -0.430 -0.43% +0.430 0.675 0.430 0.46 kp= IPNO 12 [PNo12 {Por] (0.430R (0.4612 (0:675 =](http://img.homeworklib.com/questions/abc6be60-f0c8-11eb-9ef5-573becc1fe0a.png?x-oss-process=image/resize,w_560)
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W 14-2 Problem 2 (3 pts) The atmospheric oxidation of nitric oxide was studied at 184°C...
2 attempts left Check my work Be sure to answer all parts. Nitric oxide (NO) reacts...
2 attempts left Check my work Be sure to answer all parts. Nitric oxide (NO) reacts with molecular oxygen as follows: 2NO(g) + O2(g) → 2NO2(g) Initially NO and O2 are separated in two different chambers connected by a valve. When the valve is opened, the reaction quickly goes to completion. Determine what gases remain at the end and calculate their partial pressures. Assume that the temperature remains constant at 25°C. Initial conditions are as follows: NO: 3.97 L, 0.500...
Answer is A 47. The oxidation of nitric oxide to nitrogen dioxide is 2NO(g) + O2(g)...
Answer is A
47. The oxidation of nitric oxide to nitrogen dioxide is 2NO(g) + O2(g) + 2NO2(g) If 100.0 mL of NO (at STP) reacts with 400.0 mL of O2 at STP, calculate the partial pressure of NO2 in the final reaction mixture. A) 0.222 atm B) 0.333 atm C) 0.286 atm 0.250 atm E) 1.00 atm
Question 3 0.6 pts Nitric oxide is made from the oxidation of ammonia. What mass of...
Question 3 0.6 pts Nitric oxide is made from the oxidation of ammonia. What mass of nitric oxide can be made from the reaction of 8.00 g NH3 with 17.0 g O2 4 NH3(g) +5 O2(g) 4 NO(g) 6 H20(g)
The oxidation of nitric oxide NO + 02 =NO2 takes place in an isothermal batch reactor....
The oxidation of nitric oxide NO + 02 =NO2 takes place in an isothermal batch reactor. The reactor is charged with a mixture containing 20.0 volume percent NO and the balance air at an initial pressure of 380 kPa (absolute). (a) Assuming ideal-gas behavior, determine the composition of the mixture (component mole fractions) and the final pressure (kPa) if the conversion of NO is 90%. (b) Suppose the pressure in the reactor eventually equilibrates (levels out) at 360 kPa. What...
7. Gas Law Problem Nitric oxide (NO) reacts with molecular oxygen 2NO(g) + O2(g) → 2NO2(g)....
7. Gas Law Problem Nitric oxide (NO) reacts with molecular oxygen 2NO(g) + O2(g) → 2NO2(g). Initially, equal volumes of the reactant gases are separated in a 2.0 L container. The pressure of the NO is 1.25 atm, while the pressure of the O2 is 0.85 atm. What are the partial pressures of the gases once the reaction has gone to completion. Assume the temperature remains constant at 0°C.
Nitric oxide (NO) reacts with molecular oxygen as follows: 2NO(g) + O2(g) 2N02(8) Initially NO and...
Nitric oxide (NO) reacts with molecular oxygen as follows: 2NO(g) + O2(g) 2N02(8) Initially NO and O2 are separated in two different chambers connected by a valve. When the valve is opened, the reaction quickly goes to completion. Determine what gases remain at the end and calculate their partial pressures. Assume that the temperature remains constant at 25°C. Initial conditions are as follows: NO: 3.92 L, 0.500 atm 02:2.01 L, 1.00 atm Pro- atm Proz=10.333 |
No more information is provided...please help a) The rate constant for the oxidation of nitric oxide...
No more information is provided...please help
a) The rate constant for the oxidation of nitric oxide by ozone is 2x10 14 molecule cm2 sec. Write the reaction and set up the rate equation. The rate constant for a competing reaction in which nitric oxide is oxidized by O2 to form nitrogen dioxide is 2x 10-38 molecule2cm'sec. Write the reaction and set up the rate equation. c) For typical concentrations encountered in morning smog episodes, namely 40 ppb for ozone and...
At 2200 degrees C gaseous nitrous oxide is synthesized from nitrogen gas and oxygen gas where...
At 2200 degrees C gaseous nitrous oxide is synthesized from nitrogen gas and oxygen gas where the equilibrium constant is 0.050 for the reaction. Calculate the equilibrium pressures of NO if nitrogen gas has an initial pressure of 7.46 am and oxygen gas is initially at 0.95 atm N2(g) + O2(g) - 2NO (ICE)
Question 6 2 pts Nitric oxide, NO, is made from the oxidation of NH3, and the...
Question 6 2 pts Nitric oxide, NO, is made from the oxidation of NH3, and the reaction is represented by the equation: 4NH3 + 502 → 4NO + 6H20 What mass of NO can be produced from 6.82 g of NH3? 3.87 g NO 12.0 g NO 6.82 g NO 18.0 g NO 15.0 g NO
Be sure to answer all parts. At 430°C, the equilibrium constant (Kp) for the reaction 2NO(g)+O2()s 2NO2(g) is 1.5 x...
Be sure to answer all parts. At 430°C, the equilibrium constant (Kp) for the reaction 2NO(g)+O2()s 2NO2(g) is 1.5 x 105. In one experiment, the initial pressures of NO, O2, and NO are 6.3 x 103 atm, 1.9 x 10-2 atm, and 0.18 atm, respectively. Calculate Op and predict the direction that the net reaction will shift to reach equilibrium. What is Qp for the experiment? 4.29 In which direction will the system proceed to reach equilibrium? The reaction will...
2 attempts left Check my work Be sure to answer all parts. Nitric oxide (NO) reacts with molecular oxygen as follows: 2NO(g) + O2(g) → 2NO2(g) Initially NO and O2 are separated in two different chambers connected by a valve. When the valve is opened, the reaction quickly goes to completion. Determine what gases remain at the end and calculate their partial pressures. Assume that the temperature remains constant at 25°C. Initial conditions are as follows: NO: 3.97 L, 0.500...
Answer is A
47. The oxidation of nitric oxide to nitrogen dioxide is 2NO(g) + O2(g) + 2NO2(g) If 100.0 mL of NO (at STP) reacts with 400.0 mL of O2 at STP, calculate the partial pressure of NO2 in the final reaction mixture. A) 0.222 atm B) 0.333 atm C) 0.286 atm 0.250 atm E) 1.00 atm
Question 3 0.6 pts Nitric oxide is made from the oxidation of ammonia. What mass of nitric oxide can be made from the reaction of 8.00 g NH3 with 17.0 g O2 4 NH3(g) +5 O2(g) 4 NO(g) 6 H20(g)
The oxidation of nitric oxide NO + 02 =NO2 takes place in an isothermal batch reactor. The reactor is charged with a mixture containing 20.0 volume percent NO and the balance air at an initial pressure of 380 kPa (absolute). (a) Assuming ideal-gas behavior, determine the composition of the mixture (component mole fractions) and the final pressure (kPa) if the conversion of NO is 90%. (b) Suppose the pressure in the reactor eventually equilibrates (levels out) at 360 kPa. What...
7. Gas Law Problem Nitric oxide (NO) reacts with molecular oxygen 2NO(g) + O2(g) → 2NO2(g). Initially, equal volumes of the reactant gases are separated in a 2.0 L container. The pressure of the NO is 1.25 atm, while the pressure of the O2 is 0.85 atm. What are the partial pressures of the gases once the reaction has gone to completion. Assume the temperature remains constant at 0°C.
Nitric oxide (NO) reacts with molecular oxygen as follows: 2NO(g) + O2(g) 2N02(8) Initially NO and O2 are separated in two different chambers connected by a valve. When the valve is opened, the reaction quickly goes to completion. Determine what gases remain at the end and calculate their partial pressures. Assume that the temperature remains constant at 25°C. Initial conditions are as follows: NO: 3.92 L, 0.500 atm 02:2.01 L, 1.00 atm Pro- atm Proz=10.333 |
No more information is provided...please help
a) The rate constant for the oxidation of nitric oxide by ozone is 2x10 14 molecule cm2 sec. Write the reaction and set up the rate equation. The rate constant for a competing reaction in which nitric oxide is oxidized by O2 to form nitrogen dioxide is 2x 10-38 molecule2cm'sec. Write the reaction and set up the rate equation. c) For typical concentrations encountered in morning smog episodes, namely 40 ppb for ozone and...
At 2200 degrees C gaseous nitrous oxide is synthesized from nitrogen gas and oxygen gas where the equilibrium constant is 0.050 for the reaction. Calculate the equilibrium pressures of NO if nitrogen gas has an initial pressure of 7.46 am and oxygen gas is initially at 0.95 atm N2(g) + O2(g) - 2NO (ICE)
Question 6 2 pts Nitric oxide, NO, is made from the oxidation of NH3, and the reaction is represented by the equation: 4NH3 + 502 → 4NO + 6H20 What mass of NO can be produced from 6.82 g of NH3? 3.87 g NO 12.0 g NO 6.82 g NO 18.0 g NO 15.0 g NO
Be sure to answer all parts. At 430°C, the equilibrium constant (Kp) for the reaction 2NO(g)+O2()s 2NO2(g) is 1.5 x 105. In one experiment, the initial pressures of NO, O2, and NO are 6.3 x 103 atm, 1.9 x 10-2 atm, and 0.18 atm, respectively. Calculate Op and predict the direction that the net reaction will shift to reach equilibrium. What is Qp for the experiment? 4.29 In which direction will the system proceed to reach equilibrium? The reaction will...
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