3. The temperature-dependence of the equilibrium constant was observed for a particular reaction. A plot of InK. (y-axis) versus 1/T (x-axis) produced a straight line with the equa- tion y = 4304x 11. Refer to the Introduction and the Data Sheet to determine a) the enthalpy change (AH) of the reaction (in kJ/mol). b) the entropy change (AS) of the reaction (in J/K• mol).

3. The temperature-dependence of the equilibrium constant was observed for a particular reaction. A plot of InK. (y-axis) versus 1/T (x-axis) produced a straight line with the equa- tion y = 4304x 11. Refer to the Introduction and the Data Sheet to determine a) the enthalpy change (AH) of the reaction (in kJ/mol). b) the entropy change (AS) of the reaction (in J/K• mol).

Principles of Modern Chemistry

8th Edition

ISBN:9781305079113

Author:David W. Oxtoby, H. Pat Gillis, Laurie J. Butler

Publisher:David W. Oxtoby, H. Pat Gillis, Laurie J. Butler

Chapter14: Chemical Equilibrium

Section: Chapter Questions

Problem 87AP

See similar textbooks

Similar questions

The equilibrium constant for the reaction 2CrO42(aq)+2H+(aq)Cr2O72(aq)+H2O is 31014 . What must the pH be so that the concentrations of chromate and dichromate ion are both 0.10 M?
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 Ksp for a very insoluble salt is 4.2 * 10-47 at 298 K. What is ∆G° for the dissolution of the salt in water?
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.
1. What is the Gibbs energy for the given reaction at the specified temperature and with 2M NO₂, 1 M O₂, and 2 M NO). Is the reaction spontaneous or nonspontaneous?1.1 Using the given in 1, what is the value of the reaction quotient? Is it less than, greater than or equal to K and what does it mean?2. If the total change in internal energy of the system is -88.18 kJ, what is the value for work? Is it done on the system or done by the system?
At 2300 K, the equilibrium constant for the formation of NO (g), is K = 1.7 x 10-3. N2 (g) + O2 (g) NO 2 NO (g) (a) The analysis shows that the concentrations of N2 and O2 are both 0.25 mol L-1, and that ofNO is 0.0042 mol L-1, under certain conditions. Is the system in balance? In caseaffirmative or negative, substantiate your answer.(b) If the system is not in equilibrium, in which direction should the reaction proceed?(c) When the system is in equilibrium, what are the equilibrium concentrations?
Jen is running an experiment about the dissociation of HI gas. She writes her equation to be: 2HI (g) = H2 (g) + I2 (g) Then she looks up the literature and databases. She finds that the equillibrium constant of HI formation from hygrogen and iodine gasses is 0.4 under the standard condition. She does not want to change her reaction direction because many other calculations such as enthalpy, entropy, and free energy are based on the reaction direction she has picked. What the equillibrium constant she should use under the standard condition? Keq = ______
2.The equilibrium constant for the reaction of decomposition of AB3 (AB3(g) = A(g) + 3B (g)) is K = [A][B]^3/[AB3] where and are the concentrations of A, B and AB3 respectively. Use the properties of logarithms to obtain the -log as a function of logK, log and .
In the gas phase reaction 2 A(g) + B(g) ⇋ 3 C (g) + 2 D (g), it was found that when 1.00 mol A, 2.00 mol B and 1.00 mol D were mixed and allowed to come to equilibrium at 25oC, the resulting mixture contained 0.9 mol C at a total pressure of 1.00 bar. Calculate the mole fractions of each species , Kx is , Kp is and is
One reaction has a standard Gibbs energy of -320 kJ mol-1 and a second reaction has a standard Gibbs energy of -55 kJ mol-1. What is the ratio of their equilibrium constants at 300 K?
The decomposition vapor pressure of NH4Cl at 421°C was 618 kPa and increased to 1215 kPa at 459°C.NH4Cl(k) NH3(g) + HCl(g)(a) the equilibrium constant,(b) the standard reaction Gibbs energy,(c) standard enthalpy,(d) Calculate the standard decomposition entropy, all at 421°C.Note that steam behaves like an ideal gas and that ΔH° and ΔS° are independent of temperature in the given range.Assume it is.
The reaction of ozone in the atmosphere and nitric oxide has a reaction enthalpy and reaction entropy of -199 kJ mol-1 and -4.1 J K-1 mol-1, respectively. What is its reaction Gibbs energy at 25 °C? O3(g) + NO(g) → NO2(g) + O2(g) -200 kJ mol-1 1220 kJ mol-1 -1420 kJ mol-1 -198 kJ mol-1