4. The equilibrium constant of a reaction A(g) = 2B(g) was found to fit the expression 4375 +1.75 InT(K) - 1.50 x 10ST2(K) T(K) InK = 6.043 between 0°C and 100°C. a) Find the degree of dissociation of A at 25°C when the total pressure is 2 bar. b) What must be the total pressure at 25°C for 10% dissociation of A. c) Calculate the standard reaction entalpy, entropy and the standard reaction Gibbs energy at 25°C. d - (In x) dx 1

4. The equilibrium constant of a reaction A(g) = 2B(g) was found to fit the expression 4375 +1.75 InT(K) - 1.50 x 10ST2(K) T(K) InK = 6.043 between 0°C and 100°C. a) Find the degree of dissociation of A at 25°C when the total pressure is 2 bar. b) What must be the total pressure at 25°C for 10% dissociation of A. c) Calculate the standard reaction entalpy, entropy and the standard reaction Gibbs energy at 25°C. d - (In x) dx 1

Chemistry: The Molecular Science

5th Edition

ISBN:9781285199047

Author:John W. Moore, Conrad L. Stanitski

Publisher:John W. Moore, Conrad L. Stanitski

Chapter12: Chemical Equilibrium

Section12.5: Using Equilibrium Constants

Problem 12.7CE

See similar textbooks

Similar questions

In the gas-phase reaction A + B ⇋ C + 2 D, it was found that, when 2.00 mol A, 1.00 mol B, and 3.00 mol D were mixed and allowed to come to equilibrium at 25 °C, the resulting mixture contained 0.79 mol C at a total pressure of 1.00 bar. Calculate (i) the mole fractions of each species at equilibrium, (ii) K, and (iii) ΔrG⦵.
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.
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.
At T = 298.15 K, the equilibrium constant of a reaction is 3.876926675 x 10-6. What is the equilibrium constant at T = 305.15 K if Hrxn at 293.15 K to 323.15 K is equal to -23.40 kJ/mol?
For the reactionHCO2H (g) → CO (g) + H2O (g)At 321.1 K, the following concentrations are observed:[HCO2H (g)] = 0.0470[CO (g)] = 0.737[H2O (g)] = 0.885a) What is the reaction quotient for this system?
For the gas-phase reaction 2SO2 + O2 =2SO3, the observed mole fractions for a certain equilibriummixture at 1000 K and 1767 torr are xSO2 = 0.310, xO2 = 0.250, and xSO3 = 0.440. Calculate KP at 1000 K
In the reaction 2A (g) + B(g)==>2C(g) + D(g), 3.00 mol A was mixed with 2 mol of B and 0.5 mol of D. The system was allowed to come to equilibrium. At equilibrium, 1.2 mol of C was present at a total pressure of 1 bar. Calculate the mole fractions of each species at equilibrium, K, and ΔGr at 298 K.
Consider the reaction: H2(g) + I2(g)⇌2 HI(g)H2(g) + I2(g)⇌2 HI(g) A reaction mixture at equilibrium at 600 K contains 0.170 bar H2, 0.120 bar I2, and 1.26 bar HI. A second reaction mixture, also at 600 K, contains 0.135 bar each of H2 and I2 and 1.10 bar of HI. Is the second mixture at equilibrium? If not, what will be the partial pressure of HI when the reaction reaches equilibrium at 600 K?
C(S) + H2O(G) < =>co(G) + h2 (G) HAS A MIXTURE OF GASES AT 800 ^oc. kp = 14.1. IF WE START SOLID CARBON AT 0.1 MOL H2O IN 1 LITER VESSEL. and at 25 degree kp = 1.7 x 10 ^-21, Is this reaction endotermic or exothermic to produce maximum amount of CO and h2 at equilibrium should the pressure of the system increase or decrease.?
For the reaction PCl5(g)⇌ PCl3(g) + Cl2(g), the equilibrium constantKc = 1.1 x 10-2 at 400 K. What is the equilibrium constant for the reactionPCl3(g) + Cl2(g)⇌ PCl5(g) at 400 K?
Pentene (C5H10) reacts with ethanoic acid to form pentyl ethanoate, the equilibrium CH3CO2H + C5H10 ➡ CH3CO2C5H11 being established when a solution of 0.020 moles of pentene and 0.010 moles of acetic acid in 600cm3 of an inert solvent was allowed to reach equilibrium at 150C, 0.0090 moles of pentyl ethanoate was formed. How many moles of pentene and ethanoic acid were present in the solution after equilibrium had been attained?
For the reaction: N2O4(g) ↔ 2NO2 (g)Between 298 and 900 K, it is true that: Kp = αTbe-c / T(a) Deduce expressions for ∆Gr°, ∆rH° and ∆rS° as a function of temperature, for this reaction.(b) Calculate ∆Gr°, ∆rH° and ∆rS° for the reaction at 600 K, knowing that α = 1.09x1013; b = -1.304 and c = 7307