Question

The equilibrium constant for the dissociation of oxygen, O 2 ↔ 2 O, at 1400 K...

The equilibrium constant for the dissociation of oxygen, O 2 ↔ 2 O, at 1400 K is 8.8 x 10 -13 . Calculate the degree of dissociation (extent of reaction) for P total = 1 Pa.

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
The equilibrium constant for the reaction A ↔ B is K=350.0 at 310 K. The rate...
The equilibrium constant for the reaction A ↔ B is K=350.0 at 310 K. The rate constant for the reaction A → B at 310 K is 200 s-1. What is the rate cosntant for the reaction B → A at 310 K?
For an equilibrium reaction 2 A + 3 B ↔ 2 C, the equilibrium constant Kc...
For an equilibrium reaction 2 A + 3 B ↔ 2 C, the equilibrium constant Kc = 1.6×103. For the reaction C ↔ A + 3/2 B, the value of equilibrium constant, Kc', is [Y]. (Fill in the blank. Show the value only. Report with proper number of significant figures and do not use scientific notation.) -------- 4. A sealed 1.0 L flask is charged with 0.500 mol of I2 and 0.500 mol of Br2. An equilibrium reaction ensues: I2(g)...
a) Calculate the equilibrium constant at 17 K for a reaction with ΔHrxno = 10 kJ...
a) Calculate the equilibrium constant at 17 K for a reaction with ΔHrxno = 10 kJ and ΔSrxno = -100 J/K. (Don't round until the end. Using the exponent enlarges any round-off error.) b) Calculate the equilibrium constant at 146 K for the thermodynamic data in the previous question (Notice that Keq is larger at the larger temperature for an endothermic reaction) c) Calculate the equilibrium constant at 43 K for a reaction with ΔHrxno = 10 kJ and ΔSrxno...
At 365 K and a total equilibrium pressure of 0.985 atm, the fractional dissociation of CH2Cl2...
At 365 K and a total equilibrium pressure of 0.985 atm, the fractional dissociation of CH2Cl2 is 0.850 for the reaction 2CH2Cl2(g) <----> CH4(g) + CCl4(g) This means that 850 of every 1000 molecules of CH2Cl2 originally present have dissociated. Calculate the equilibrium constant in terms of pressures, Kp. Kp = _______
At 1,500 K, the equilibrium constant for the reaction below is Kc=0.0819. Br2(g) --> 2 Br(g)...
At 1,500 K, the equilibrium constant for the reaction below is Kc=0.0819. Br2(g) --> 2 Br(g) What is the percent dissociation of Br2 at 1,500 K, if the initial concentration of Br2 is 2.25 mol/L? Give your answer accurate to two significant figures. Do not include the % sign as part of your answer. Hint: If the initial concentration of Br2 is Co and the concentration of Br2 decreases by x (because of dissociation), then the percent dissociation of Br2...
At 1,600 K, the equilibrium constant for the reaction below is Kc = 0.215. Br2(g) ⇌...
At 1,600 K, the equilibrium constant for the reaction below is Kc = 0.215. Br2(g) ⇌ 2 Br(g) What is the percent dissociation of Br2 at 1,600 K, if the initial concentration of Br2 is 2.25 mol L−1 ?
At a certain temperature the equilibrium constant, K c, equals 0.11 for the reaction: 2 ICl(g)...
At a certain temperature the equilibrium constant, K c, equals 0.11 for the reaction: 2 ICl(g) ↔ I2(g) + Cl2(g). What is the equilibrium concentration of ICl if 0.25 mol of I2 and 0.25 mol of Cl2 are initially mixed in a 2.0-L flask?
The equilibrium constant for the reaction N2 + O2<--> 2NO is 1.69 × 10^?3 at 2300...
The equilibrium constant for the reaction N2 + O2<--> 2NO is 1.69 × 10^?3 at 2300 K. A mixture consisting of 2 mol of nitrogen and 1.0 mol of oxygen is heated to 2300 K at 1 bar and allowed to come to equilibrium. Calculate the mole fraction of NO at equilibrium.
Calculate the equilibrium constant at 37 K for a reaction with ΔHrxno = 10 kJ and...
Calculate the equilibrium constant at 37 K for a reaction with ΔHrxno = 10 kJ and ΔSrxno = 100 J/K. Calculate the equilibrium constant at 129 K for the thermodynamic data in the previous question.
The equilibrium constant, Kp, equals 3.40 for the isomerization reaction: cis-2-butene ↔ trans-2-butene. If a flask...
The equilibrium constant, Kp, equals 3.40 for the isomerization reaction: cis-2-butene ↔ trans-2-butene. If a flask initially contains 0.250 atm of cis-2-butene and 0.145 atm of trans-2-butene, what is the equilibrium pressure of each gas?