The equilibrium constant (K) fordecomposition of gaseous H,O;the63.1H;Oe = Hu) +Oe is related to degree of2(),dissociation (a) at a total pressure P, given by:-a³p!/2(1) Kp =(1 +a) (2 + a) '/²%3D3/2(2) Кр -(1 – a) (2 + a) '/23/2,2(3) Kp=(1 – a) (2 + a) '/²(4) Kp =a?pl/23/2,1/2(1 – a) (2 + a) '/2

Answered: Image /qna-images/answer/0f4f7a0b-6344-4f68-a517-af054631bfc3.jpg

for the The equilibrium constant (K) decomposition of gaseous H,O; 63. H,O = Hye) + 1 O2) is related to degree of dissociation (a) at a total pressure P, given by:- 3,1/2 a°p!/2 (1) Kp = (1+a) (2 + a) '/2 3,3/2 (2) Кр — %3D (1 – a) (2 + a) '/² 3/2. a2p? (1 – a) (2 + a) '/2 (3) Kp (4) Kp: a 3/2p1/2 (1- a) (2+ a) /2

for the The equilibrium constant (K) decomposition of gaseous H,O; 63. H,O = Hye) + 1 O2) is related to degree of dissociation (a) at a total pressure P, given by:- 3,1/2 a°p!/2 (1) Kp = (1+a) (2 + a) '/2 3,3/2 (2) Кр — %3D (1 – a) (2 + a) '/² 3/2. a2p? (1 – a) (2 + a) '/2 (3) Kp (4) Kp: a 3/2p1/2 (1- a) (2+ a) /2

Chemistry: Principles and Reactions

8th Edition

ISBN:9781305079373

Author:William L. Masterton, Cecile N. Hurley

Publisher:William L. Masterton, Cecile N. Hurley

Chapter12: Gaseous Chemical Equilibrium

Section: Chapter Questions

Problem 36QAP: At a certain temperature, K=0.29 for the decomposition of two moles of iodine trichloride, ICl3(s),...

See similar textbooks

Similar questions

. The solubility product of magnesium carbonate, MgCO3, has the value Ksp = 6. 82 × 10−6at 25°C. How many grams of MgCO3will dissolve in 1.00L of water?
A mixture consiting of 1.000 mol H2O(g) and 1.000 mol CO(g) is placed ina reaction vessel of volume 10.00 L at 800. K. At equilibrium, 0.665 mol CO2(g) is present as a result of the reaction CO (g) + H2O (g)⇋ CO2(g)+H2(g). What are the equilibrium concentrations for all substances?
The equilibrium constant for the gas-phase isomerization of borneol, C10H17OH, to isoborneol at 503 K is 0.106. A mixture consisting of 6.70 g of borneol and 12 .5 g of isoborneol in a container of volume 5.0 dm3 is heated to 503 K and allowed to come to equilibrium. Calculate the mole fractionsof the two substances at equilibrium.
A mixture consiting of 1.000 mol H2O(g) and 1.000 mol CO(g) is placed ina reaction vessel of volume 10.00 L at 800. K. At equilibrium, 0.665 mol CO2(g) is present as a result of the reaction CO (g) + H2O (g)⇋ CO2(g)+H2(g). What are the value of KC at 800. K?
The equilibrium constant Kc for C + CO2 <=> 2CO is 1.9 at 1000 K and 0.133 at 298K. How many grams of C are consumed?
A reaction mixture that consisted of 0.20 mol N2(g) and 0.20 mol H2(g) was introduced into a reactor of volume 25.0 L and heated. At equilibrium, 5.0% of the nitrogen gas had reacted. What is the value of the equilibrium constant KC for the reaction N2(g) + 3H2(g) ⇋ 2 NH3(g) at this temperature?
If the equilibrium constant for the reaction A+ B ⇌ C is reported as 0.432, what would be the equilibrium constant for the reaction written as C ⇌ A+ B?
The equilibrium constant for the gas-phase isomerization of borneol (C10H17OH) to its isomer isoborneol at 503 K is 0.106. A mixture consisting of 7.50 g of borneol and 14.0 g of isoborneol in a container of volume 5.0 dm3 is heated to 503 K and allowed to come to equilibrium. Calculate the mole fractions of the two substances at equilibrium.
Estimate the temperature at which the equilibrium constant for CuSO4 ⋅ 5 H2O(s) → CuSO4(s) + 5 H2O(g) becomes 1; assume pH2O = 1 bar.
The following synthesis reaction was conducted at 325K: A2(g) + 3B2(g) ⇌ 2AB3(g). At this temperature, KP = 5.49 x 10-6. In a 3.00L flask, 0.175atm of A2(g) and 0.410atm of B2(g) are added and allowed to reach equilibrium. Calculate the pressure of AB3(g) in the system (in atm).
What would be the equilibrium temperature if you drop 5.0 g of brass (Cp= 0.38 J/g-°C, initially at 68°C) and 3.5 g of aluminum (Cp = 0.9 J/g-°Cinitially at 83°C) into 105 g of water (Cp = 4.184 J/g-°C,initially at 23°C)?
The phase diagram for SO2 is shown here. (a) What doesthis diagram tell you about the enthalpy change in thereaction SO2(l) ---->SO2(g)? (b) Calculate the equilibriumconstant for this reaction at 100 °C and at 0 °C.(c) Why is it not possible to calculate an equilibrium constantbetween the gas and liquid phases in the supercriticalregion? (d) At which of the three points marked in reddoes SO2(g) most closely approach ideal-gas behavior?(e) At which of the three red points does SO2(g) behaveleast ideally?