Question

Consider the following equilibrated system: 2NO2(g) 2NO(g) + O2(g). If the Kp value is 0.604, find...

Consider the following equilibrated system: 2NO2(g) 2NO(g) + O2(g). If the Kp value is 0.604, find the equilibrium pressure of the O2 gas if the NO2 gas pressure is 0.520 atm and the PNO is 0.300 atm at equilibrium.x

Homework Answers

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
Consider the following equilibrated system: 2NO2(g) 2NO(g) + O2(g). If the Kp value is 0.997, find...
Consider the following equilibrated system: 2NO2(g) 2NO(g) + O2(g). If the Kp value is 0.997, find the equilibrium pressure of the O2 gas if the NO2 gas pressure is 0.520 atm and the PNO is 0.300 atm at equilibrium. I really need a good explaination toward the end when you actually solve for [02] because I get that far but don't know how to reaarange my equation.
At 1000 K, a sample of pure NO2 gas decomposes: 2NO2(g) ⇌ 2NO(g) + O2(g) The...
At 1000 K, a sample of pure NO2 gas decomposes: 2NO2(g) ⇌ 2NO(g) + O2(g) The equilibrium constant, KP, is 158. Analysis shows that the partial pressure of O2 is 0.45 atm at equilibrium. Calculate the pressure of NO and NO2 in the mixture
34. Consider the reaction 2NO(g) + O2(g) ⇆ 2NO2(g) At a certain temperature, an equilibrium mixture...
34. Consider the reaction 2NO(g) + O2(g) ⇆ 2NO2(g) At a certain temperature, an equilibrium mixture consists of 0.0230 mole O2, 0.0470 mole NO, and 0.919 mole of NO2. Calculate KP for the reaction, given that the total pressure is 0.200 atm. KP =
For the equilibrium 2NO2(g) ⇌ 2NO(g) + O2(g), Kp = 2.0 × 10-2 at 365oC. Suppose...
For the equilibrium 2NO2(g) ⇌ 2NO(g) + O2(g), Kp = 2.0 × 10-2 at 365oC. Suppose 0.0600 mol NO(g), 0.0150 mol O2(g), and 1.60 mol NO2(g) are added to a rigid 2.00-L flask. What is ΔG?
Consider the following reaction and corresponding value of Kc 2NO(g)+O2(g)⇌2NO2(g)Kc=5.4×1013 at 25∘C What is the value...
Consider the following reaction and corresponding value of Kc 2NO(g)+O2(g)⇌2NO2(g)Kc=5.4×1013 at 25∘C What is the value of Kp at this temperature? Express your answer using two significant figures.
The decomposition of NO2 2NO2(g) → 2NO(g) + O2(g) is second-order in NO2. Given that the...
The decomposition of NO2 2NO2(g) → 2NO(g) + O2(g) is second-order in NO2. Given that the half-life for the inital concentration of NO2 equal to 0.848 M is 221 s, find the concentration of NO2 after 663 s.
Find ΔG∘rxn for the reaction: N2O(g)+NO2(g)→3NO(g) Use the following reactions with known ΔG values: 2NO(g)+O2(g)→2NO2(g)ΔG∘rxn=−71.2kJ N2(g)+O2(g)→2NO(g)ΔG∘rxn=+175.2kJ...
Find ΔG∘rxn for the reaction: N2O(g)+NO2(g)→3NO(g) Use the following reactions with known ΔG values: 2NO(g)+O2(g)→2NO2(g)ΔG∘rxn=−71.2kJ N2(g)+O2(g)→2NO(g)ΔG∘rxn=+175.2kJ 2N2O(g)→2N2(g)+O2(g)ΔG∘rxn=−207.4kJ
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.
the following data were obtained for the reaction, 2NO2(g)-->2NO (g) + O2. Times   (NO2) 0   0.8333...
the following data were obtained for the reaction, 2NO2(g)-->2NO (g) + O2. Times   (NO2) 0   0.8333 20   0.4167 40   0.2778 60   0.2083 c) what is the reaction order with respect to NO2? explain D) write the rate law for this equation
7. Consider the following reaction: 2NO2 (g) -> 2NO(g) + O2 (g) rate = k[NO2]^2 When...
7. Consider the following reaction: 2NO2 (g) -> 2NO(g) + O2 (g) rate = k[NO2]^2 When the initial concentration of NO2 is 100 mM, it takes 55 s for 90% of the NO2 to react. Calculate the rate constant. a) 0.042 M–1·s–1 d) 1.6 ´ 10–3 M–1·s–1 b) 1.8 ´ 10–5 M–1·s–1 e) 0.13 M–1·s–1 c) 1.6 M–1·s–1 I am getting d.) but i am not sure, please confirm