Question

At a given temperature, Kp = 19 for the reaction, N2O4(g) <=> 2 NO2(g) For which...

At a given temperature, Kp = 19 for the reaction,
N2O4(g) <=> 2 NO2(g)
For which system is the value of Kp = 361?

Please show work so I can figure out what I am doing wrong. Thank you!

Science   Chemistry   
0 0
Add a commentTranscribed image text
Next >

Homework Answers

Answer #1

For given transformation,

N2O4(g) <======> 2 NO2(g)

Equilibrium constant Kp can be written as,

Kp = (PNO2)2/(PN2O4)

And

Kp =19 given

So, (PNO2)2/(PN2O4) = 19

Squaring on both side we get,

[(PNO2)2/(PN2O4)]2 = (19)2

(PNO2)4/(PN2O4)2 = 361

(PNO2)4/(PN2O4)2 = Pk’

This expression indicate, the stoichiometric transformation,

2N2O4(g) <======= > 4NO2(g)

Hence for this 2N2O4(g) <======= > 4NO2(g) system Kp =361.

=========================================

0 0
Know the answer?
Your Answer:

Post as a guest

Your Name:

What's your source?

Earn Coins

Coins can be redeemed for fabulous gifts.

Log In

Sign Up

Not the answer you're looking for?
Ask your own homework help question
Similar Questions
At a particular temperature, Kp=0.22 for the reaction N2O4(g)=2NO2(g) A flask containing only NO2 at an...
At a particular temperature, Kp=0.22 for the reaction N2O4(g)=2NO2(g) A flask containing only NO2 at an initial pressure of 5.8 atm is allowed to reach equilibrium. Calculate the equilibrium partial pressures of the gases.
At a particular temperature, Kp = 0.26 for the reaction below. N2O4(g) equilibrium reaction arrow 2...
At a particular temperature, Kp = 0.26 for the reaction below. N2O4(g) equilibrium reaction arrow 2 NO2(g) (a) A flask containing only N2O4 at an initial pressure of 4.9 atm is allowed to reach equilibrium. Calculate the equilibrium partial pressures of the gases. b) he volume of the container in part (a) is decreased to one-half the original volume. Calculate the new equilibrium partial pressures.
Calculate the equilibrium concentrations of N2O4 and NO2 at 25 ∘C if the initial concentrations are...
Calculate the equilibrium concentrations of N2O4 and NO2 at 25 ∘C if the initial concentrations are [N2O4]= 0.0210 M and [NO2]= 0.0340 M. The equilibrium constant Kc for the reaction N2O4(g)⇌2NO2(g) is 4.64×10−3 at 25 ∘C. 1) Calculate the equilibrium concentration of N2O4. 2) Calculate the equilibrium concentration of NO2. I have worked through this problem several times and keep getting the wrong answer. I think I'm making a math error along the way. Could you show as much work...
1- Above what temperature is the following reaction spontaneous? N2O4(g) ↔ 2 NO2(g) ΔH° = 57.24...
1- Above what temperature is the following reaction spontaneous? N2O4(g) ↔ 2 NO2(g) ΔH° = 57.24 kJ/mol ΔS° = 175.5 J/mol∙K Group of answer choices 326 K 53.2 K 307 K 273 K 2- Predict the sign on ΔG for the following reaction when PI2 = PH2 = 0.01 atm and PHI = 1.0 atm. H2(g) + I2(g) ↔ 2 HI(g) ΔG° = -15.94 kJ/mol & Kp,298K = 620 Group of answer choices ΔG = 0 ΔG > 0 ΔG...
9.Consider the following reaction: NO(g) + SO3(g) ⇌ NO2(g) + SO2(g) A reaction mixture initially contains...
9.Consider the following reaction: NO(g) + SO3(g) ⇌ NO2(g) + SO2(g) A reaction mixture initially contains 0.86 atm NO and 0.86 atm SO3. Determine the equilibrium pressure of NO2 if Kp for the reaction at this temperature is 0.0118 please show as much detail as you can!
The equilibrium constant (KP) is 0.17 at a particular temperature for the reaction: N2O4(g) ⇌ 2NO2(g)...
The equilibrium constant (KP) is 0.17 at a particular temperature for the reaction: N2O4(g) ⇌ 2NO2(g) Given the following sets of initial conditions, what is the net change that must occur for the reaction to reach equilibrium? Does the reaction shift left to reach equilibrium, does the reaction shift right to reach equilibrium or is the reaction at equilibrium at these initial concentrations so no net change will occur? RIGHT, LEFT, or EQUILIBRIUM 1. PNO2 = 0.252 atm, PN2O4 =...
At 25 C, the equilibrium constant for the reaction 2A(g) <-> B(g) + C(g) is Kp...
At 25 C, the equilibrium constant for the reaction 2A(g) <-> B(g) + C(g) is Kp = 0.0833. If the three gases are mixed in a rigid container having partial pressure of 2.58, 1.71 and 0.307 atm for A, B and C, respectively, is the system at equilibrium? Potential answers: The forward reaction must proceed to establish equilibrium, The volume of the container must be known to answer the question, The concentrations of all substances must be known to answer...
Figure out what is wrong with each questions and answers: 1.) For the reaction 2A(g)+3B(g)⇌C(g) Kc...
Figure out what is wrong with each questions and answers: 1.) For the reaction 2A(g)+3B(g)⇌C(g) Kc = 78.0 at a temperature of 239 ∘C .Calculate the value of Kp. Ans: Kp=2.50 x 10^-5 2.) For the reaction X(g)+2Y(g)⇌3Z(g) Kp = 1.38×10−2 at a temperature of 81 ∘C .Calculate the value of Kc. Ans: Kc = 1.38 x 10^-2 3.) For the reaction 2CH4(g)⇌C2H2(g)+3H2(g) K = 0.145 at 1590 ∘C . What is Kp for the reaction at this temperature? Ans:...
A) Calculate KP at 298 K for the reaction NO(g)+1/2O2(g)→NO2(g) assuming that ΔH∘R is constant over...
A) Calculate KP at 298 K for the reaction NO(g)+1/2O2(g)→NO2(g) assuming that ΔH∘R is constant over the interval 298-600K. NOTE: I can tell you for sure the following answers are wrong: 7.2*10^10; 1.38*10^-11; 10.35; 14.65 B: Calculate KP at 475 K for this reaction assuming that ΔH∘R is constant over the interval 298-600 K. My prof told me to use: ln(K2/K)=-ΔH/(1/T2-1/T1) but it is not working for me NOTE: the following answers are wrong: 1.16*10^7; 6.26*10^6; 102
Calculate KP at 298 K for the reaction NO(g)+12O2(g)→NO2(g) assuming that ΔH∘R is constant over the...
Calculate KP at 298 K for the reaction NO(g)+12O2(g)→NO2(g) assuming that ΔH∘R is constant over the interval 298-600 K. Calculate KP at 496 K for this reaction assuming that ΔH∘R is constant over the interval 298-600 K. Do you expect KP to increase or decrease as the temperature is increased to 600. K? to increase to decrease
ADVERTISEMENT
Need Online Homework Help?

Get Answers For Free
Most questions answered within 1 hours.

Ask a Question
ADVERTISEMENT