CaCO3 (s) dissociates in a closedsystem according to the reaction:CaCO, (s) = CaO(s) +CO, (g)32Assuming the reaction is inthermodynamic equilibrium, thedegree(s) of freedom. F =whenAssCaCO,(s) dissociates in a closed system according to the reaction:CaCO(s) Cao(s) + CO2(g)peraAAssuming the reaction is in thermodynamic equilibrium, the degree(s) of freedom. F-eta20

Temperature, pressure, and concentration are related by the following formula which associates the…

Answered: CaCO3 (s) dissociates in a closed…

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...

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7. FREE GIBBS ENERGY RELATING TO KP ⚫ Consider the decomposition of barium carbonate BaCO3(s) BaO (s)+CO (g) Use data in Appendix A to calculate the equilibrium pressure of CO at a) 298 K and b) 1100 K.
Calcium chloride has the following solubility reaction: CaCl₂ (s) Ca²+ (aq) + 2Cl(aq) Given the following molar enthalpies and entropies, what would happen to the solubility by increasing temperature? Compound CaCl₂(s) Ca²+ (aq) CI (aq) Ob) solubility decreases AHf (kJ/mol) a) more information is needed c) solubility increases -795.8 -542.96 -167.16 d) temperature has no effect on solubility ASf (J/mol-K) -55.2 56.5 -46.8
Estimate the ΔG for the following reaction. What is ΔG at 298 K if p = 0.25 bar for each gaseous substance in the above Reaction. a) 2 H2(g) + O2(g) 2 H2O(l) b) C(s, graphite) + 2 H2(g) CH4(g). H2 (g) 0 O2 (g) 0 H2O (l) -237.1 C(s, graphite) 0 CH4 (g)
Consider the reaction: 2H₂O (1) --> 2H₂(g) + O₂(g) Decrease in entropy (delta S 0)
Be sure to answer all parts. Using the data in the table, calculate Kp and AG for this reaction at 25°C. PC15(g) = PC13(g) + Cl2(g) AG" f Initial Partial Substance Pressure (atm) (kJ/mol) Cl2(s) 0.358 PCI3(g) -286 0.213 PCI5(g) -325 0.00320 Кр- X 10 AG= kJ/mol
Consider the following reaction with equilibrium constant 0.02532 at 25 oC. 2 A (g) + B (g) -------- 3 C(g) Determine free energy change for a mixture of 0.75 mol A, 1.20 mol C and 3.40 mol B in a 5.0-L vessel at 25 oC considering the above reaction in forward direction.
Estimate the temperature in K at which the reaction will become nonspontaneous.
Compound NH4HCO3(s) NH3(g) CO2(g) H20(E) AG°; (kJ/mol) -665.9 -16.45 -394.4 -237.1 Consider the given reaction: NH3(g) + CO2(g) + H20(4) = NH4HCO3(s) Calculate AG at 298K for this reaction when the pressures of NH3 and CO2 are 0.52 atm and 0.31 atm, respectively. 22.5 kJ -26.7 kJ -13.4 kJ O 13.4 kJ O -22.5 kJ
O ENTROPY AND FREE ENERGY Using reaction free energy to predict equilibrium composition D 3/5 Consider the following equilibrium: 2NOC1 (g) - 2NO (g)+ Cl, (g) AG" =41. kJ Now suppose a reaction vessel is filled with 2.68 atm of nitrosyl chloride (NOCI) and 3.74 atm of chlorine (Cl,) at 227. °C. Answer the following questions about this system: rise Under these conditions, will the pressure of Cl, tend to rise or fall? fall Is it possible to reverse this tendency by adding NO? In other words, if you said the pressure of Cl, will tend to rise, can that yes be changed to a tendency to fall by adding NO? Similarly, if you said the no pressure of Cl, will tend to fall, can that be changed to a tendency to rise by adding NO? If you said the tendency can be reversed in the second question, calculate the minimum pressure of NO needed to reverse it. | atm Round your answer to 2 significant digits. II

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