When barium carbonate dissociates according to the reaction, BacO; (s) = Bao (s) + CO2 (g) the pressure of CO2 g) in equilibrium with the solid phases is 7.0x10-2 bar at 1400 K and 0.37 bar at 1500 K. Use this information to calculate A,H°, A,G° and 4,5° at 298.15 K. You may assume that 4,H° is independent of temperature.

When barium carbonate dissociates according to the reaction, BacO; (s) = Bao (s) + CO2 (g) the pressure of CO2 g) in equilibrium with the solid phases is 7.0x10-2 bar at 1400 K and 0.37 bar at 1500 K. Use this information to calculate A,H°, A,G° and 4,5° at 298.15 K. You may assume that 4,H° is independent of temperature.

Chemistry

10th Edition

ISBN:9781305957404

Author:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste

Publisher:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste

Chapter1: Chemical Foundations

Section: Chapter Questions

Problem 1RQ: Define and explain the differences between the following terms. a. law and theory b. theory and...

See similar textbooks

Similar questions

Calcium oxide can decompose into calcium and oxygen according to 2CaO(s)2Ca(s) + O2(g) Calculate the standard Gibbs energy change for this at 298 K given that At(CaO(s)) = -635,1 kJ mol ¹, S(CaO(s)) = 39.7 J mol¹K¹ AP(Ca(s)) = 0, S(Ca(s)) = 41.4 J mor¹ K¹, AP(O₂(g)) = 0, and S(O2(g)) = 205 J mol¹ K¹ Answer in kJ mol
A mixture of isobutylene ((CH3)2CCH2, 0.400 bar partial pressure) and HCI (0.600 bar partial pressure) is heated at 500.0 K. The equilibrium constant K for the gas- phase thermal decomposition of tert- butyl chloride ((CH3);CCI) is 3.45 at 500.0 K. (CH3);CCI(g) = (CH3)2CCH2(g) + HCI(g) 1 3 Calculate the value of Kc 4 6. C 7 8 9 +/- х 100
NOBr(g) at 1 bar pressure is introduced into a evacuated chamber according to the equilibrium equation give below, it dissociates; 2NOBr(g) <=> 2NO(g) + Br2(g) at 25 degrees Celsius equilibrium is reached, the partial pressure is 0.60 bar of the NOBr. At 25 degrees Celsius what is the equilibrium constant for this reaction. Chose the most correct answer. a) 0.012 b) 0.062 c) 0.089 d)1.34
Part A The value of K, for nitrous acid (HNO,) at 25 °Cis 4.5 x 10 4 Part B Part C What is the value of AG at equilibrium? Express your answer using one significant figure. AG = 0 kJ Submit Previous Answers v Correct By definition, the Gibbs free energy of a reaction is zero when it is at equilibrium. Forward and reverse reactions continue to occur dynamically, but there is Part D What is the value of AG when [H'] = 5.1 x 10 2 M. [NO,] = 6.2 x 10 4M and (HNO2] = 0.21 M? Express your answer using three significant figure. ? AG = kJ Submit Previous Answers Request Answer X Incorrect; Try Again; 5 attempts remaining
For the following reaction: A(g) + B(g) = 2 C(a) Calculate the magnitude of K, (don't report the units) assuming the following composition at equilibrium: PA = 0.438 bar PB = 0.716 bar Pc = 0.122 bar
Calculate the equilibrium constant at 37°C for the reaction Glucose +6O2 + 36ADP + 36Phosphate -> 6CO2 + 42H2O + 36ATP Change in G°= -423kcal/mole of Glucose
What is the A,G for the following reaction (in kJ mol ¹) at 298 K? 2 Si (s) + 3 H2(g) Si₂H6 (g) 1 The conditions for this reaction are: PH2 = 1.21 bar PsizH6 = 0.5 bar. You will also need to use Appendix II in your textbook (containing standard Gibbs energies of formation). A copy of Appendix II has also been posted on eClass. Please use the method of Gibbs energy of formation to calculate ArG" if needed. For partial credit, enter the value of "Q" for this reaction. Answer:
Give detailed Solution...don't give Handwritten answer
Dinitrogen tetroxide is 18.46 per cent dissociated at 25°C and 1.00 bar in the equilibrium N2O4(g) ⇌ 2NO2(g). Calculate K at (i) 25°C, (ii) 100°C given that ΔrH° = +56.2 kJ mol−1 over the temperature range.
Dinitrogen tetroxide is 18.46 per cent dissociated at 25°C and 1.00 bar in the equilibrium N2O4(g) ⇌ 2NO2(g). Calculate K at (i) 25°C, (ii) 100°C given that ΔrH° = +56.2 kJ mol−1 over the temperature range.
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 Kp. [.960]
At 25 °C, the equilibrium partial pressures for the reaction 3 A(g) + 4 B(g) 2C(g) + 2D(g) were found to be PA = 4.67 atm, På = 5.73 atm, Pc = 5.60 atm, and Pp = 5.84 atm. What is the standard change in Gibbs free energy of this reaction at 25 °C? kJ mol privacy policy contact us help terms of use 6:11 PM about us careers 3/25/202