Question

ozone reacts completely with no producing No2 and O2. A 11.02L vessel is filled with 1.246...

ozone reacts completely with no producing No2 and O2. A 11.02L vessel is filled with 1.246 mol of NO and 1.246 O3 at 383.0 K. Find the partial pressure in the flask at the end of the reaction.

Homework Answers

Answer #1

                 O3      +     NO ----------->   NO2 + O2

t=0         1.246         1.246                 0           0

after reaction        0             0                  1.246         1.246

Pno2= PO2 = nNO2RT/V = (1.246x 0.0821x 383)/11.02 =3.555 atm each

Total pressure = 3.55 x2 = 7.1 atm

Know the answer?
Your Answer:

Post as a guest

Your Name:

What's your source?

Earn Coins

Coins can be redeemed for fabulous gifts.

Not the answer you're looking for?
Ask your own homework help question
Similar Questions
Solve: 2 NO2 (g) + O3 (g) → N2O5 (g) + O2 (g)      ∆Hº = -198...
Solve: 2 NO2 (g) + O3 (g) → N2O5 (g) + O2 (g)      ∆Hº = -198 kJ mol-1RXN     ∆Sº = -168 J K-1        Ozone reacts with nitrogen dioxide according to the equation above. State and explain how the spontaneity of this reaction will vary with increasing temperature. Substance ∆Hºf (kJ mol -1) O3 (g) 143 N2O5 (g) 11
Carbon monoxide at a pressure of 1200 mmHg reacts completely with O2 at a pressure of...
Carbon monoxide at a pressure of 1200 mmHg reacts completely with O2 at a pressure of 590 mmHg in a sealed vessel to produce CO2. What is the final pressure in the flask? (in mmHg)
2 NO2(g) <---------> 2 NO(g) + O2(g) Starting with pure NO2 , the flask is heated...
2 NO2(g) <---------> 2 NO(g) + O2(g) Starting with pure NO2 , the flask is heated and he partial pressure of O2 at equlibrium is 0.133 am. Calculate the partial pressures of NO and NO2 at equlibrium and the total pressure in the flask at equlibrium. PNO ____________________atm PNO2____________________atm Ptotal____________________atm
1)A reaction vessel at 27 ∘C contains a mixture of SO2(P= 3.10 atm ) and O2(P=...
1)A reaction vessel at 27 ∘C contains a mixture of SO2(P= 3.10 atm ) and O2(P= 1.00 atm ). When a catalyst is added the reaction 2SO2(g)+O2(g)⇌2SO3(g) takes place. At equilibrium the total pressure is 3.85 atm. -Find the value of Kc. 2)A sample of SO3 is introduced into an evacuated sealed container and heated to 600 K. The following equilibrium is established: 2SO3(g)⇌2SO2(g)+O2(g). The total pressure in the system is found to be 3.0 atm and the mole fraction...
A reaction of importance in the formation of smog is that between ozone and nitrogen monoxide...
A reaction of importance in the formation of smog is that between ozone and nitrogen monoxide described by O3(g)+NO(g)⟶O2(g)+NO2(g) The rate law for this reaction is rate of reaction=?[O3][NO] Given that ?=2.26×106 M−1⋅s−1 at a certain temperature, calculate the initial reaction rate when [O3] and [NO] remain essentially constant at the values [O3]0=7.82×10−6 M and [NO]0=7.71×10−5 M, owing to continuous production from separate sources. initial reaction rate: M⋅s−1 Calculate the number of moles of NO2(g) produced per hour per liter...
The rate constant for the decomposition of gaseous NO2 to NO and O2 is 4.7/(M?s) at...
The rate constant for the decomposition of gaseous NO2 to NO and O2 is 4.7/(M?s) at 383 ?C. Consider the decomposition of a sample of pure NO2 having an initial pressure of 752mmHg in a 5.50L reaction vessel at 383 ?C. It is a second order reaction. B. What is the initial rate of formation of O2 in g/(L?s)? USE TWO SIGNIFICANT FIGURES C. What is the mass of O2 in the vessel after a reaction time of 2.00min ?
The decomposition of NO2(g) occurs by the following bimolecular elementary reaction. 2 NO2(g) → 2 NO(g)...
The decomposition of NO2(g) occurs by the following bimolecular elementary reaction. 2 NO2(g) → 2 NO(g) + O2(g) The rate constant at 273 K is 2.3 ✕ 10-12 L/mol · s, and the activation energy is 111 kJ/mol. How long will it take for the concentration of NO2(g) to decrease from an initial partial pressure of 4.0 atm to 2.4 atm at 451 K? Assume ideal gas behavior.
The rate constant for the reaction NO2 + O3 --> NO3 + O2 was determined over...
The rate constant for the reaction NO2 + O3 --> NO3 + O2 was determined over a range of 40 K, with the following results: T (K) k(M-1s-1) 203 4.14x105 213 7.30x105 223 1.22x106 233 1.96x106 243 3.02x106 A. Determine the activation energy for the reaction. B. Calculate the rate constant of the reaction at 300 K.
Chlorine gas reacts with fluorine gas to form chlorine trifluoride. Cl2(g)+3F2(g)→2ClF3(g) A 2.00 L reaction vessel,...
Chlorine gas reacts with fluorine gas to form chlorine trifluoride. Cl2(g)+3F2(g)→2ClF3(g) A 2.00 L reaction vessel, initially at 298 K, contains chlorine gas at a partial pressure of 337 mmHg and fluorine gas at a partial pressure of 784 mmHg . Part A What is the pressure of ClF3 in the reaction vessel after the reaction? Part B What is the total pressure in the reaction vessel after the reaction? So, I've tried this problem, but I end up having...
NO2 is one of the atmospheic pollutants produced by automobiles. It is formed when the high...
NO2 is one of the atmospheic pollutants produced by automobiles. It is formed when the high temperature in the internal combustion engine causes atmospheric N2 and O2 to combine to produce NO, which then reacts with more O2 to give NO2. This pollutant ultimately is converted to HNO3. Aproposed equation for this convertion at 2989 K is O3(g) +2NO2(g)+H2O(g)--------- 2HNO3(aq)+O2(g). Calculate the enthalpy for the conversion reaction