At T = 25 degrees Celsius, the reaction No2 <-> 2NO +O2 has an equilibrium constant K=5.0*10^-13. Suppose the container is filled with NO2 at an initial pressure of 0.25 atm. Calculate the partial pressure of NO at equilibrium

67,647 results

Chemistry

At T = 25 degrees Celsius, the reaction No2 <-> 2NO +O2 has an equilibrium constant K=5.0*10^-13. Suppose the container is filled with NO2 at an initial pressure of 0.25 atm. Calculate the partial pressure of NO at equilibrium

Chemistry

At T = 25 degrees Celsius, the reaction No2 <-> 2NO +O2 has an equilibrium constant K=5.0*10^-13. Suppose the container is filled with NO2 at an initial pressure of 0.25 atm. Calculate the partial pressure of NO at equilibrium

chemistry

a flask is charged with 2.00 atm of nitrogen dioxide and 1.00 atm of dinitrogen tetroxide at 25 degrees celsius and allowed to reach equilibrium.when equilibrium is established, the partial pressure of NO2 has decreased by 1.24 atm. (a) what are the partial pressures of NO2 ...

chemistry

Liquid Nitrogen tetroxide, N2O4(l), was used as a fuel in Apollo missions to the moon. In a closed container the gas N2O4(g) decomposes to nitrogen dioxide, NO2(g). The equilibrium constant,k, for this reaction is 0.87 at 55 degrees Celsius. A vessel filled with N2O4(g) at ...

Chemistry

Consider this equilibrium: N2O4(g) + heat NO2(g). Initially, a 1.0 L container is filled with 2.0 mol of NO2. As the system approaches equilibrium, what happens to the rate of reaction of NO2 breaking down?

Chemistry

Consider this equilibrium: N2O4(g) + heat NO2(g). Initially, a 1.0 L container is filled with 2.0 mol of NO2. As the system approaches equilibrium, what happens to the rate of reaction of NO2 breaking down?

Chemistry

2 NO(g) + O2 (g) <==> 2 NO2 (g) Given that Kp=7.96×1012 for the reaction above and the following starting conditions: Initial Concentrations p(NO)=0.775 atm p(NO2)=0.000 atm p(O2)=0.789 atm Determine the equilibrium concentration of NO2.

chem

A flask is charged with 1.596 atm of N2O4(g) and 1.008 atm of NO2(g) at 25°C, and the following equilibrium is achieved. N2O4(g)-> 2 NO2(g) After equilibrium is reached, the partial pressure of NO2 is 0.504 atm. (a) What is the equilibrium partial pressure of N2O4? for ...

Chemistry

At 700 K, the equilibrium constant for the reaction NO2(g) « 2NO(g) + O2(g) is Kc = 4.79×10-3 (M), and the rate constant for the reaction 2NO(g) + O2(g) ® NO2(g) is k = 3.13×10^3 M^-2s^-1. What is the rate constant for the reaction NO2(g) ® 2NO(g) + O2(g) at this ...

Equilibrium

The following reaction has an equilibrium constant (Keq) of 160. 2 NO2(g) <--> 2 NO(g) + O2(g) What will be the reaction quotient (Q) and in which direction will the reaction proceed if the partial pressure of NO2 is 5.0*10^-4 atm, NO is 0.080 atm, and O2 is 0.020 atm? ...

chemisty

The initial concentration of NO2 in a closed container is 0.750M. At equilibrium the concentration of O2 is 0.125M. What are the concentrations of NO2 and NO at equilibrium? 2NO2 (aq) ==== 2NO (aq) + O2 (aq)

CHM

Given the initial concentrations of 0.10 atm NO2 and 0.10 atm N2O4 in a 1.0 L flask, what will be the equilibrium partial pressure of NO2? N2O4(g)=2NO2 Kp=0.660at319K Choose one answer. a. 0.10 atm b. 0.31 atm c. 0.045 atm d. 0.72 atm e. 0.19 atm

CHEMISTRY

The equilibrium constant for the reaction, SO2(g)+ NO2(g) <----> NO(g)+ SO3(g) has been experimentally determined as a function of temperature. The results are presented in the table below. T (°F) KC 285 662 752 156 842 93.4 932 59.6 1022 40.2 If 0.0791 ft3 SO2, 0.158 ...

Chemistry

A container at room temperature is filled with equal moles of O2(g), NO2(g) and He(g). The gases slowly leak through a pinhole in the container. After some gas has effused, which relationship is true about the partial pressures of the gas remaining in the container? a) P He &...

chemistry

I need help. I have no clue how to find this. A flask is charged with 1.680 atm of N2O4(g) and 1.220 atm of NO2(g) at 25 degrees celcius. The equilibrium reaction is N2O4 <-> 2 NO2 After equilibrium is reached, the partial pressure of NO2 is 0.550 (a) What is the ...

(1-16)Chemistry - Science

Consider the reaction: SO2 (g) + NO2 (g) ==> SO3 (g) + NO (g) At T = 1000 K, where the reaction is exothermic with an equilibrium constant K = 9.00 The reaction vessel is charged initially with all four gases, each at a pressure of 0.5 atm. After equilibrium is achieved, ...

Chemistry

Chemistry equilibrium? Consider the reaction 2NO(g) + O2(g) = 2NO2(g) at 430C an equilibrium mixture consists of 0.020 mole of O2, 0.040 mole of NO, and 0.96 mole of NO2. Calculate Kp for this reaction given that the total pressure is 0.20 atm. I used PV=nRT to find the volume...

chemistry

Consider the reaction 2 NO2 (g) ⇌ 2 NO (g) + O2 (g). If the initial partial pressure of NO2 (g) is 3.0 bar, and x is the equilibrium pressure of O2 (g), what is the correct equilibrium relation?

chemical equilibrium

At a certain temperature, Kc = 0.914 for the reaction NO2 (g) + NO (g) <----> N2O (g) + O2 (g) Equal amounts of NO and NO2 are to be placed in a 5.00 L container until the N2O concentration at equilibrium is 0.050 M. How many moles of NO and NO2 must be placed in the ...

(1-17)Chemistry - Science

Consider the reaction: SO2 (g) + NO2 (g)  SO3 (g) + NO (g) At T = 1000 K, where the reaction is exothermic with an equilibrium constant K = 9.00 If the reaction vessel is instead charged initially with SO3(g) and NO(g), each at a partial pressure of 0.500 atm, the ...

CHEMISTRY

1.0 mol of nitrogen oxide NO and 1.0 mol of oxygen were mixed in a container and heated to 450 oC. At equilibrium the number of moles of oxygen was found to be 0.70 mol. The total pressure in the vessel was 4.0 atm. Calculate the value of Kp for the reaction: 2NO (g) + O2 (g) ...

Pchem

2 NO2(g) N2(g) + 2 O2(g) The ¥ÄH¡Æ for the reaction above is -66.4 kJ. The system is initially at equilibrium. What happens if NO2 is added to the reaction mixture at constant temperature and volume? (Select all that apply.) And here's the options. The reaction absorbs ...

chemistry

At 2200 degrees celsius,kp=0.050 for the reaction: n2(g)+O2(g) ->2NO(g) <- What is the partial pressure of NO in equilibrium with N2 and O2 that were placed in a flask at initial pressures of .80 and .20 atm, respectively?

Chemistry Equilibrium

For the reaction NO2(g) + NO(g) N2O(g) + O2(g) Kc = 0.914. Equal amounts of NO and NO2 are to be placed into a 5.00 L container until the N2O concentration at equilibrium is 0.0446 M. How many moles each of NO and NO2 must be placed into the container?

Chemistry

Consider the reaction for the production of NO2 from NO: 2 NO(g) + O2(g) = 2 NO2(g) a)If 84.8L of O2(g), measured at 35 degrees Celsius and 632mm Hg, is allowed to react with 158.2g of NO, find the limiting reagent. b) If 97.3L of NO2 forms, measured at 35 degrees Celsius and ...

chemistry

An equilibrium mixture contains N2O4, (P= 0.30 ) and NO2 (P= 1.1 ) at 350 K. The volume of the container is doubled at constant temperature. Calculate the equilibrium pressure of when the system reaches a new equilibrium. Calculate the equilibrium pressure of NO2 when the ...

Chemistry

I am having great difficulty with the following questions. Any and all help will be greatly appreciated. I have read the chapter and even looked up online tutorials. I still do not understand it. 2 NO (G) + O2 (G) > 2 NO2 (G) Write the equilibrium constant expression for ...

Chemistry HELP!!!!

Nitric oxide (NO) reacts with molecular oxygen as follows: 2NO(g) + O2(g) ¨ 2NO2(g) Initially NO and O2 are separated as shown below. When the valve is opened, the reaction quickly goes to completion. Determine what gases remain at the end of the reaction and calculate ...

Chemistry

Nitric oxide (NO) reacts with molecular oxygen as follows: 2NO(g) + O2(g) ¨ 2NO2(g) Initially NO and O2 are separated as shown below. When the valve is opened, the reaction quickly goes to completion. Determine what gases remain at the end of the reaction and calculate ...

chemistry

2 NO2(g) N2(g) + 2 O2(g) The ΔH° for the reaction above is -66.4 kJ. The system is initially at equilibrium. What happens if N2 is added to the reaction mixture at constant temperature and volume? The reaction absorbs energy. The reaction releases energy. [NO2] increases...

science

The equilibrium constant for the gas phase reaction N2O4 ⇀↽ 2 NO2 at a certain temperature is K = 0.0466. If the initial concentrations are [N2O4] = 1.0 M, [NO2] = 0.0 M, what are the final concentrations of [N2O4] and [NO2], respectively? 1. 1.0 M ; 0.22 M 2. 0.8 ...

AP Chem

At a particular temperature, Kp = 0.25 for the following reaction. N2O4(g) 2 NO2(g) (a) A flask containing only N2O4 at an initial pressure of 5.3 atm is allowed to reach equilibrium. Calculate the equilibrium partial pressures of the gases. (b) A flask containing only NO2 at ...

chem 12

1.00 mol of N2O4 and 1.00 mol of NO2 are placed in an 800 mL container. Calculate the initial concentrations of each gas. N2O4= 1.25 mol/L NO2=1.25 mol/L When equilibrium is reached, the concentration of NO2 increases by 0.50mol/L. Calculate the equilibrium NO2 and N2O4 If I ...

Chemistry

SO2(g) + NO2(g) SO3(g) + NO (g) At a given temperature, analysis of an equilibrium mixture found [SO2] = 4.00 M, [NO2] = 0.500 M, [SO3] = 3.00 M, and [NO] = 2.00 M. (a) What is the new equilibrium concentration of NO when 1.50 moles of NO2 are added to the equilibrium mixture...

Chemistry

Under the appropriate conditions, NO forms NO2 and N2O: 3NO(g) <--> N2O(g) + NO2(g) Use the values for delta G naught for the following reactions to calculate the value of Kp for the above reaction at 500.0 C 2NO(g) + O2(g) <--> 2NO(g) delta g=-69.7 kJ 2N2O(g) <...

Chemistry

Hydrazine, N2H4 can be made (on paper) by reaction of molecular nitrogen and molecular hydrogen, 2 H 2 ( g ) + N 2 ( g ) --> N 2 H 4 ( g ) and suppose that the equilibrium constant Kp has the value 1×10^–3. (a) A stoicheometric mixture of H2 and N2 is placed in a ...

chemistry

Calculate each of these equilibrium concentrations based on the reaction below. 2 NO(g) + O2(g) 2 NO2(g) K = 1.71 1012 (a) [NO] = 0.0048 M; [O2] = 0.000057 M; [NO2] = ? (b) [NO] = 0.0026 M; [O2] = 0.000023 M; [NO2] = ?

chemistry

Calculate each of these equilibrium concentrations based on the reaction below. 2 NO(g) + O2(g) 2 NO2(g) K = 1.71 1012 (a) [NO] = 0.0048 M; [O2] = 0.000057 M; [NO2] = ? (b) [NO] = 0.0026 M; [O2] = 0.000023 M; [NO2] = ?

Chemistry

For a gaseous reaction, standard conditions are 298 K and a partial pressure of 1 atm for all species. For the reaction 2NO(g) + O2(g) --> 2NO2(g) the standard change in Gibbs free energy is ΔG° = -69.0 kJ/mol. What is ΔG for this reaction at 298 K when the ...

Chemistry

Nitric oxide (NO) reacts with molecular oxygen as follows: 2NO(g) + O2(g) ¨ 2NO2(g) Initially NO and O2 are separated as shown below. When the valve is opened, the reaction quickly goes to completion. Determine what gases remain at the end of the reaction and calculate ...

Chemistry

When a sample of NO2(g) (849.9 grams) is placed in 390.0 L reaction vessel at 961.0 K and allowed to come to equilibrium the mixture contains 248.2 grams of NO(g). What is the concentration (mol/L) of NO2(g)? 2NO2(g) = 2NO(g)+O2(g) I keep getting .0212 or .04736. This is what ...

Chemistry

A piece of Na metal undergoes a complete reaction with H2O (l0 to produce sodium hydroxide and hydrogen. If 24.0 g of Na in a 3.50 L container is reacted with an excess amount of water at 25 degrees Celsius, calculate the total pressure (in atm) in the 3.50 L container when ...

CHEMISTRY

A chemist studying the equilibrium N2O4(g)<----->2NO2(g) controls the temperature so that keq ( equilibrium constant)= 0.028. At one equilibrium position, the concentration of N2O4 is 1.5 times greater than the concentration of NO2. Find the concentrations of the two ...

Chemistry

For the reaction NO2(g) + NO(g) = N2O3(g) If at particular temperature, K was 575 and equilibrium concentration of N2O3(g) was 2.5 M, calculate the equilibrium concentrations of NO2(g) and NO(g) if they both had the same initial concentrations. i have my table layed out like...

Chemistry

Dinitrogen tetroxide decomposes according to N2O4 (g) = 2NO2 (g) In a certain experiment, N2O4(g) at an initial pressure of 0.554 bar is introduced into an empty reaction container; after equilibrium is established, the total pressure is 0.770 bar. A quantity of NO2(g) is ...

Chemistry Equilibrium

At 200 °C, Kc = 1.4 x 10-10 for the reaction N2O(g) + NO2(g) 3NO(g) If 0.174 mol of N2O and 0.337 mol NO2 are placed in a 4.00 L container, what would the NO concentration be if this equilibrium were established?

Chem

The initial concentration for the compounds involved in the reaction displayed were determined to be [NO2(g)] = 1.243 mol/L, [N2O4(g)] = 0.2578 mol/L. Calculate the value of the equilibrium constant (Kc) at 500.0 K if the equilibrium concentration of NO2(g) was 0.7629 mol/L. ...

Chemistry

When 442 mg of NO2 is confined to a 150. mL reaction vessel and heated to 300°C, it decomposes by a second-order process. In the rate law for the decomposition of NO2, k = 0.54 1/(M·s). A) what is the initial reaction rate? B) what is the reaction rate if the mass of NO2 ...

College Chemistry

Given the following equilibrium constants, Ka (NH4^+)=5.6*10^-10 Kb (NO2^-)=2.2*10^-11 Kw=1.00*10^-14 determine the equilibrium constant for the reaction below at 25*C. NH4^+(aq)+NO2^-(aq)f HNO2(aq)+NH3(aq)

chemistry

The following system is at equilibrium with [N2O4] = 0.55 M and [NO2] = 0.25 M. If an additional 0.10 M NO2 is added to the reaction mixture with no change in volume, what will be the new equilibrium concentration of N2O4?      N2O4(g) 2 NO2(g)

Chem 2

The following system is at equilibrium with [N2O4] = 0.55 M and [NO2] = 0.25 M. If an additional 0.10 M NO2 is added to the reaction mixture with no change in volume, what will be the new equilibrium concentration of N2O4? N2O4(g) 2 NO2(g)

Chemistry Honors

A 0.25 mol sample of n204 dissociates and comes to equilibrium in a 1.5 L flask at 100 degrees C. The reaction is N2O4 > 2 NO2. The Kc at 100 degrees C is 0.36. What are the equilibrium concentrations of NO2 and N2O4?

Chemistry

For the following reaction 2NO2 -> 2NO +O2 is second order reaction. If the initial concentration of NO2 is 0.098M and the initial rate of disappearance is 2.72e-3 M/sec , what is the value of the rate constant?

Chemistry

92.01 grams of N2O4 (g) is placed in a container and allowed to dissociate. N2O4 (g) --> 2NO2 (g) The mixture of N2O4 and NO2 resulting from the reaction occupies 36.0 liters at a total pressure of 773 mmHg and 45 °C. A. Let x equal the moles of N2O4 that dissociate. How ...

chemistry

I also had a problem with this type of questionthe initial pressure of NOCl(g) is 4.329 atm, calculate the % of NOCl(g) left over after the reaction reaches equilibrium according to the balanced equation. The value of Kp at 400.0 °C is 1.99. The initial pressure of the ...

chemistry

Which of the following equations correctly describes the relationship between the rate at which NO2 and Cl2 are consumed in the following reaction? 2 NO2(g) + Cl2(g) → 2 NO2Cl(g) A. -d(NO2)/dt = 1/2 [d(Cl2)/dt] B. -d(NO2)/dt = 2 [d(Cl2)/dt] C. -d(NO2)/dt = 2 [-d(Cl2)/dt...

science

Which of the following equations correctly describes the relationship between the rate at which NO2 and Cl2 are consumed in the following reaction? 2 NO2(g) + Cl2(g) → 2 NO2Cl(g) A. -d(NO2)/dt = 1/2 [d(Cl2)/dt] B. -d(NO2)/dt = 2 [d(Cl2)/dt] C. -d(NO2)/dt = 2 [-d(Cl2)/dt...

Chemistry

Determine the value of the equilibrium constant,Kgoal , for the reaction N2(g)+O2(g)+H2(g)<=> (1/2)N2H4(g) + NO2(g) Kgoal=? by making use of the following information: 1.N2(g)+O2(g)<=>2NO(g), K1=4.1010x10^-31 2.N2(g)+2H2(g)<=>N2H4(g), K2=7.40x10^-26 3.2NO(g)+...

AP Chemistry

Dinitrogen pentoxide (N2O5) decomposes in chloroform as a solvent to yield NO2 and O2. The decomposition is first order with a rate constant at 45 degrees Celsius of 1.0*10^-5 s^-1.Calculate the partial pressure of O2 produced from 1.00 Liter of 0.600 M N2O5 solution at 45 ...

Chemistry!!!!

1. For a reaction mechanism to be plausible, what 2 criteria must be met? 2. The reaction between CO and NO2 to produce NO and CO2 is thought to occur in 2 steps. NO2 + NO2 ====> NO + NO3 NO3 + CO =====> NO2 + CO2 The experimental rate law is, R=k[NO2]2 Write the ...

Chemistry!!!!

1. For a reaction mechanism to be plausible, what 2 criteria must be met? 2. The reaction between CO and NO2 to produce NO and CO2 is thought to occur in 2 steps. NO2 + NO2 ====> NO + NO3 NO3 + CO =====> NO2 + CO2 The experimental rate law is, R=k[NO2]2 Write the ...

chemistry

For reactions in solution, molar concentrations are usually used in equilibrium constant expressions (designated by K or Kc). In gases, partial pressures can also be used (designated by Kp). Equilibrium partial pressures of NOCl, NO and Cl2 in a container at 300 K are 1.2 atm...

chemistry

Under the appropriate conditions, NO forms NO2 and N2O: 3NO(g) <--> N2O(g) + NO2(g) Use the values for delta G naught for the following reactions to calculate the value of Kp for the above reaction at 500.0 C 2NO(g) + O2(g) <--> 2NO(g) delta g=-69.7 kJ 2N2O(g) <...

Chemistry Equilibrium Constant

The initial pressures for I2 (g), H2(g), and HI(g) were Pi2 = 0.100 atm, Ph2 = 0.200 atm, and Phi = 0 atm, respectively. After the system came to equilibrium, the pressure of I2 (g) became very low, PI2 = 1.00 x 10^-5 atm. Calculate the equilibrium constant Kp for this reaction

chem

at 84 degrees Celsius , a gas in a container exerts a pressure of 0.503 ATM. assuming the size of the container remains the same, at what Celsius temperature would the pressure be 1.20 atm ?

chemistry

I was having trouble with this problem. initial pressure for the compounds involved in the reaction displayed were determined to be P(CO(g)) = 0.5794 atm, P(H2O(g)) = 0.5662 atm, P(CO2(g)) = 0.7950 atm, P(H2(g)) = 0.2754 atm. Calculate the value of the equilibrium constant (Kp...

chemistry

Calculate the value of the equilibrium constant (Kp) for the reaction shown, if F(g) was found to be 96.80 % decomposed at 1000 K when its initial pressure was 4.638 atm. The initial pressure of the reaction products is 0 atm. 2F(g) = F2(g)

AP Chem

NO2 + H2 <-> NO + H2O [H2] = .30 mol/L [NO2] = .20 mol/L [NO] = [H20] = .70 mol/L @ 1000K A. What is the mole fraction of NO in the equilibrium mixture? B. Calculate Kc C. Determine Kp in terms of Kc D. If system is cooled to a lower temperature, 35% of NO is converted ...

chemistry

What effect does raising the temperature of the reaction chamber at a constant pressure have on the following reaction at equilibrium? 2NO2(g) N2O4(g) + heat A. The equilibrium shifts toward the reactants because the reverse reaction is endothermic. B. The concentration of NO2...

Chemsitry

Consider the equilibrium A(g)=2B(g)+3C(g) at 25 degrees Celsius. When A is loaded into a cylinder at 10 atm and the system is allowed to come to equilibrium, the final pressure is found to be 12.13 atm. What is the standard gibbs free energy of reaction for this reaction.

Chemistry

The equilibrium constant is 16 for the gas phase reaction SO2 + NO2 <--> SO3 + NO at a certain temperature. If 3.0 moles each of SO2 and NO2 are placed together in an empty 1.0 liter flask and the system is allowed to come to equilibrium at this temperature, what will be...

chemistry

A pressurized can of paint contains a fixed mass of gas at an internal pressure of 1.258 atm at 24.8oC. Suppose the can is able to withstand an internal pressure of 2.410 atm before it explodes. At what temperature, in degrees Celsius, will this can explode? HINT: The can is a...

chemistry

Suppose 100 mL of NO at STP is mixed with 400 mL of O2 at STP. 2 NO (g) + O2 (g)---> 2 NO2 (g) After the reaction goes to completion, what is the partial pressure of NO2 in the resulting mixture of gases at STP? I know the relation between pressure and volume is P1V1=P2V2, ...

chemistry

 If we combine nitrous oxide (NO, laughing gas) with oxygen (O2) we produce nitrogen dioxide (NO2) according to the following reaction: 2NO + O2→ 2NO2 How many grams of NO2 will be produced when 5.00 moles of NO react?

AP Chem - to Dr. Bob

I don't understand how to even start this problem: A mixture of H2(g), O2(g), and 2 mL of H2O is present in a 0.5 L rigid container at 25 degrees Celsius. The number of moles of H2 and the number of moles of O2 are equal. The total pressure is 1146 mmHg. Vapor pressure of ...

Chemistry(Please respond, thank you!)

Using this data, 2 NO(g) + Cl2(g) == 2 NOCl(g) Kc = 3.20 X 10-3 NO2(g) == NO(g) + ½ O2(g) Kc = 3.93 calculate a value for Kc for the reaction, NOCl (g) + ½ O2 (g) == NO2 (g) + ½ Cl2 (g) So I understand that 2NO + Cl2 + 1/2O2 = NO2 + 1/2 Cl2 but I do not understand how you ...

chei

.0815moles NO are reacted with .0789moles O2 gas to from NO2 gas according to the following equation: 2NO + O2 = 2NO2 determine the molar amounts of NO, O2, and NO2 after complete reaction.

chemistry

.0815moles NO are reacted with .0789moles O2 gas to from NO2 gas according to the following equation: 2NO + O2 = 2NO2 determine the molar amounts of NO, O2, and NO2 after complete reaction.

Chemistry

Nitrogen dioxide, NO2, dimerizes easily to form dinitrogen tetroxide , N2O4 : 2NO2<===>N2O4 a) Calculate Change in reaction G* and K for this equilibrium. b) Calculate the (e) (the measure of the progress of the reaction) for this equilibrium if 1.00 mol NO2 were present...

Chemistry

Dinitrogen tetroxide decomposes to nitrogen dioxide: N2O4 (g) ---> 2NO2 (g) Delta H rxn: 55.3 kJ At 298 K a reaction vessel initially containing .100 atm of N2O4. When equilibrium is reached, 58% of the N2O4 has decomposed to NO2. -What percentage of N2O4 decomposes at 350 ...

Chemistry

When the rate of the reaction 2NO+O2=2NO2 was studied, the rate was found to double when the O2 concentration alone was doubled but to quadruple when the NO concentration alone was doubled. Which of the following mechanisms accounts for these observations? a.) Step 1: NO + O2=...

chemistry

I was having trouble with this problem. initial pressure for the compounds involved in the reaction displayed were determined to be P(CO(g)) = 0.5794 atm, P(H2O(g)) = 0.5662 atm, P(CO2(g)) = 0.7950 atm, P(H2(g)) = 0.2754 atm. Calculate the value of the equilibrium constant (Kp...

Chemistry

Dinitrogen tetroxide decomposes to nitrogen dioxide: N2O4(g)→2NO2(g)ΔHorxn=55.3kJ At 298 K, a reaction vessel initially contains 0.100 atm of N2O4. When equilibrium is reached, 58% of the N2O4 has decomposed to NO2. What percentage of N2O4 decomposes at 350 K ? Assume that ...

chemistry

the following reaction has a Kp = 109 at 25 degrees C 2NO(g) + Br2(g) reversible 2NOBr(g) If the equilibrium partial pressure of Br2 is 0.0159 atm and equil pressure of NOBr is 0.0768 atm, calculate the partial pressure of NO at equlibrium. What are the steps to follow for ...

chemistry

.0815 moles NO are reacted with .0789moles O2 gas to form NO2 gas according to the following equation: 2NO +O2=2NO2 determine the molar amounts of NO, O2 and NO2 after complete reaction.

chemistry

.0815 moles NO are reacted with .0789moles O2 gas to form NO2 gas according to the following equation: 2NO +O2=2NO2 determine the molar amounts of NO, O2 and NO2 after complete reaction.

Chem

The brown color associated with photochemical smog is due to NO2(g). This is involved with the following equilibrium in the atmosphere: 2 NO2(g) <===> N2O4. Predict the signs of the enthalpy and entropy changes for this reaction. If the equation is at equilibrium should ...

Chemistry

3H2(g)+N2(g)=2NH3(g) Suppose the equilibrium constant Kp = 0.003337 for the reaction above. If the equilibrium mixture contains partial pressures H2 = 0.400 atm and N2 = 0.350 atm. What is the equilibrium partial pressure of NH3 in atm?

chem

the total pressure of n2o4 and no2 IS 1.38 atm. if kp is 6.75(25 C) calculate partial pressure of NO2 in the mixture. 2NO2<---> n2o4

Chemistry

A mixture containing the same number of moles of SO2 and O2 is placed in a 2L container at 900K. The initial pressure is 1.90Atm. A reaction occurs leading to the formation of SO3: 2SO3 + O2 <--> 2SO3 After equilibrium is established the TOTAL pressure drops to 1.60 Atm...

PChem

For the gas phase reaction 2NO2 + F2 ¨ 2NO2F, the rate constant is k= 38 dm3/mol-s at 27 oC. The reaction is first-order in NO2 and first-order in F2. A) Calculate the number of moles of NO2, F2, and NO2F after 10.0 s if 2.00 mol of NO2 is mixed with 3.00 mol of F2 in a 400...

chemistry

Nitrogen dioxide (NO2) cannot be obtained in a pure form in the gas phase because it exists as a mixture of NO2 and N2O4. At 23°C and 0.94 atm, the density of this gas mixture is 2.6 g/L. What is the partial pressure of each gas? NO2 N2O4

Chemistry

A container is filled with CO2(g) and heated to 1000K. The gas pressure at this temperature is 0.50 atm. Graphite (C) is then added to the container and some of the CO2 is converted to CO according to the reaction below. The final equilibrium total gas pressure in the flask is...

chemistry

2NO + O2 -> 2NO2 200. mL of NO at STP is reacted with 500. mL O2of at STP. Calculate the partial pressure of NO2 after the reaction goes to completion. Assume a constant volume.

Chemistry

Dinitrogen tetraoxide decomposes to give nitrogen dioxide. Calculate the equilibrium concentration of NO2 at 100oC if the equilibrium constant is 0.200 and [N2O4] = 0.800M. N2O4(g) ¡ê 2 NO2(g)

Chemistry

At 573 K, gaseous NO2(g) decomposes, forming NO(g) and O2(g). If a vessel containing NO2(g) has an initial concentration of 1.9 × 10−2 mol/L, how long will it take for 75% of the NO2(g) to decompose? The decomposition of NO2(g) is second-order in the reactant and the ...

chemistry

The pollutant NO is formed in diesel engines. The reaction fixes atmospheric nitrogen with oxygen to form NO. The reaction is: N2(g) + O2(g) = 2NO(g). If the equilibrium constant for this reaction at elevated temperatures is 5.60E-11, then what is the partial pressure of NO ...

Chemistry12

For the reaction NO2 + NO = N2O3 If at a particular temperature, K was 575 and the equilibrium concentration of N2O3 was 2.5M, calculate the equilibrium concentrations of NO2 and NO if they both had the same initial concentrations. I have this information in a table but i only...

Chemistry

The equilibrium constant Kp for the reaction below at 700°C is 0.76 atm. CCl4(g) C(s) + 2 Cl2(g) Determine the initial pressure of carbon tetrachloride that will produce a total equilibrium pressure of 1.20 atm at 700°C

Chemistry

The equilibrium constant Kp for the reaction below at 700°C is 0.76 atm. CCl4(g) --> C(s) + 2 Cl2(g) Determine the initial pressure of carbon tetrachloride that will produce a total equilibrium pressure of 1.20 atm at 700°C

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