Question

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

Science   Chemistry   
0 0
Add a commentTranscribed image text
Next >

Homework Answers

Answer #1

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
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
A) Calculate Kc for the reaction below. I2(g)⇌2I(g)Kp=6.26×10−22 (at 298 K) B) Calculate Kc for the...
A) Calculate Kc for the reaction below. I2(g)⇌2I(g)Kp=6.26×10−22 (at 298 K) B) Calculate Kc for the reaction below. CH4(g)+H2O(g)⇌CO(g)+3H2(g)Kp=7.7×1024 (at 298 K) C) Calculate Kc for the reaction below. I2(g)+Cl2(g)⇌2ICl(g)Kp=81.9 (at 298 K)
1. The equilibrium constant, Kp, for the following reaction is 4.55×10-5 at 723 K. N2(g) +...
1. The equilibrium constant, Kp, for the following reaction is 4.55×10-5 at 723 K. N2(g) + 3H2(g) 2NH3(g) If ΔH° for this reaction is -111 kJ, what is the value of Kp at 839 K? Kp= 2. The equilibrium constant, Kp, for the following reaction is 0.110 at 298 K. NH4HS(s) NH3(g) + H2S(g) If ΔH° for this reaction is 92.7 kJ, what is the value of Kp at 393 K? Kp=
The reaction below has an equilibrium constant Kp=2.2×106 at 298 K. 2COF2(g)⇌CO2(g)+CF4(g) Calculate Kp for the...
The reaction below has an equilibrium constant Kp=2.2×106 at 298 K. 2COF2(g)⇌CO2(g)+CF4(g) Calculate Kp for the reaction below. COF2(g)⇌12CO2(g)+12CF4(g)
The reaction below has an equilibrium constant of Kp=2.26×104 at 298 K. CO(g)+2H2(g)⇌CH3OH(g) A) Calculate Kp...
The reaction below has an equilibrium constant of Kp=2.26×104 at 298 K. CO(g)+2H2(g)⇌CH3OH(g) A) Calculate Kp for the reaction below. 12CH3OH(g)⇌12CO(g)+H2(g) B) Calculate Kp for the reaction below. 2CO(g)+4H2(g)⇌2CH3OH(g) C) Calculate Kp for the reaction below. 3CH3OH(g)⇌3CO(g)+6H2(g)
The reaction below has an equilibrium constant of Kp=2.26×104 at 298 K. CO(g)+2H2(g)⇌CH3OH(g) Part A Calculate...
The reaction below has an equilibrium constant of Kp=2.26×104 at 298 K. CO(g)+2H2(g)⇌CH3OH(g) Part A Calculate Kp for the reaction below. CH3OH(g)⇌CO(g)+2H2(g) K = Part B Predict whether reactants or products will be favored at equilibrium in the reaction above. Products will be favored at equilibrium. Reactants will be favored at equilibrium. Part C Calculate Kp for the reaction below. 12CO(g)+H2(g)⇌12CH3OH(g) K = Part D Predict whether reactants or products will be favored at equilibrium in the reaction above. Products...
For the reaction N2O4(g)⇌2NO2(g), ΔH0=+57.2kJmol−1 and KP=0.113 at 298 K 1) What is KP at 0∘C...
For the reaction N2O4(g)⇌2NO2(g), ΔH0=+57.2kJmol−1 and KP=0.113 at 298 K 1) What is KP at 0∘C 2) At what temperature will KP= 1.00?
1. 2CH4(g)⇌C2H2(g)+3H2(g) K = 0.160 at 1658 ∘C . What is Kp for the reaction at...
1. 2CH4(g)⇌C2H2(g)+3H2(g) K = 0.160 at 1658 ∘C . What is Kp for the reaction at this temperature? Express your answer numerically. 2. N2(g)+3H2(g)⇌2NH3(g) Kp = 4.75×10−3 at 306 ∘C . What is K for the reaction at this temperature? Enter your answer numerically. 3. Given the two reactions H2S⇌HS− + H+,   K1 = 9.12×10−8, and HS−⇌S2− + H+,   K2 = 1.52×10−19, what is the equilibrium constant Kfinal for the following reaction? S2− + 2H+⇌H2S Enter your answer numerically. 4. Given the...
Problem 6.29 (2) Part A Assuming that ΔH∘f is constant in the interval 275 K -...
Problem 6.29 (2) Part A Assuming that ΔH∘f is constant in the interval 275 K - 600. K, calculate ΔG∘ for the process (H2O, g,298→H2O, g, 597 K ). **Delta G is in the units: J*mol^-1 Part B Calculate the relative change in the Gibbs energy. Express your answer using two significant figures. **Relative change is a percentage!! Express your answer using four significant figures.
1) The equilibrium constant, Kp, for the following reaction is 0.497 at 500 K: PCl5(g) <---...
1) The equilibrium constant, Kp, for the following reaction is 0.497 at 500 K: PCl5(g) <--- ----->PCl3(g) + Cl2(g) (reversible) Calculate the equilibrium partial pressures of all species when PCl5(g) is introduced into an evacuated flask at a pressure of 1.52 atm at 500 K.   PPCl5 = _____atm PPCl3 = ______atm PCl2 = ______atm 2) The equilibrium constant, Kp, for the following reaction is 55.6 at 698 K: H2(g) + I2(g) <----- ----> 2HI(g) (reversible) Calculate the equilibrium partial pressures...
ADVERTISEMENT
Need Online Homework Help?

Get Answers For Free
Most questions answered within 1 hours.

Ask a Question
ADVERTISEMENT