DATASHEET EXPI KINETICS TO THERMODYNAMICSPART 1: EQUILIBRIUM: Ag (aq) + Fe2(aq) = Ag(s) + Fe(aq)SpeciesAH,SAG,kJ mol-¹JK-1kJ mol-1Ag (aq)73.4577.11Fe2+(aq)-87.9-113.4-84.94Ag(s)42.6Fe (aq)-47.691. Activation energy for forward reaction:2. Activation energy for reverse reaction:4. AS3. AH6. E°5. AG

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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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What is the spontaneity of the chemical system? Cu(s) + H+(aq) -> Cu2+(aq, 1M) + H2(g) standard state
18. From the following reacțions and thermal data at 25°C 3 2 Fe(s) +O:(g) 2 Fe,O:(s) ΔΗ - 196,500 cal %3D 1 2 FeO(s) + ; 0:(g) - Fe2O:(s) AH° = -67,900 cal Fe(s) + 2 H* (a = 1) = Fe++ (a = 1) + H2(g) AH° = -21,000 cal %3D %3D 1 H:(g) H* (a = 1) AHº = 0 cal %3D Hig) +0:(g) = H;0(1) AH° = -68,320 cal %3D calculate AH° of the reaction: FeO(s) + 2 H+ (a = 1) = H;0(1) + Fe++ (a = 1) %3D
a) For a reaction with AH = -152.6 kJ mol-¹ and AS°= -543.8 J K-¹ mol-¹ at 25 °C, how will AGº change if the reaction temperature is increased? Explain your answer. b) Calculate the equilibrium constant for the reaction at 80 °C, showing your working (assume AH and AS° are temperature independent).
The reaction between iron and thiocyanate ions involves this equation: Fe3+ (aq) + ScN" (aq) = FESCN2+ (aq) AH (-) kJ/mol (yellow) (colorless) (red) Match the observation with the given condition: A few drops of 1M Fe(NO3)3 has been added A. The red color of the solution intensifies. B. Yellow solution Three drops of 0.01 M AGNO3 has been added C. Colorless solution v A few drops of 0.5 M K3PO4 has been added D. The color of the solution faded to orange and yellow ppt has been observed v The system has been subjected to a boiling water bath E. turns to a more intense red color v The system has been subjected in an ice bath
In an experiment, 15 mL of 1.0 M Na2CO3 was reacted with 5 mL 2.0 M Ca(NO3)2. Calculate the AG of the reaction if it was kept at 25°C. Thermodynamic data: AH°pxn= -66 kJ/mol AS rxn= -501 J/mol-K O a. 84.23 kJ/mol O b. 65 kJ/mol O c. -83.5 kJ/mol O d. 83.3 kJ/mol
The below reaction was found to have AH = -3606 kJ mol-1 and AS = 33 J mol- K-1. What is AG for this reaction at 100.2 °C? 90,(g) + 2CH;CHCH,(g) – 6CO,(g) + 6H2O(g) Oa. -3618 kJ mol-1 Ob. -3609 kJ mol-1 Oc. -15927 kJ mol-1 Od. -3573 kJ mol-1 Oe. -3594 kJ mol-1
For the reaction 2 A(aq) <---> B(aq) + C(aq), the standard free enthalpy variation is 1.43 kJ at 25oC. The initial concentration of A is 0.541 M, the initial concentration of B is 0.343 M, and the initial concentration of C is 0.267 M. At equilibrium (we are still at 25oC), what will be the concentration of A( aq) (in mol/L)?
Use the following redox reactions and their corresponding ΔE° values: Co(s) + Pb2+(aq) ⟶ Co2+(aq) + Pb(s) ΔE° = +0.15 V Zn(s) + Co2+(aq) ⟶ Zn2+(aq) + Co(s) ΔE° = +0.48 V Which one of these chemical species is the strongest oxidizing agent? Group of answer choices Pb2+(aq) Zn(s) Co(s) Insufficient information to answer this question. Co2+(aq)
The equilibrium constant Kc for C + CO2 <=> 2CO is 1.9 at 1000 K and 0.133 at 298K. Is the reaction endothermic or exothermic?
Carbon dioxide dissolves in water to form carbonic acid. Estimate the thermodynamic equilibrium constant for this reaction using the AG; values in the table. Substance AG; (kJ/mol) H,CO, (aq) -616.1 H,O(1) -237.1 CO,(g) -394.4 K = Carbonic acid then ionizes in water (K = 4.5 x 10-7). Ignoring K2, estimate K for the overall process by which CO, and H,O form H* and HCO,. K = What is the pressure of CO, in equilibrium with carbonated water at 25 °C and pH = 4.78? Роо, atm
R = 8.314 mol-K F = 96,485 mol AG = AG° + RT · In(Q) ΔΕ - (E) · In(Q) ΔΕ. Half Reaction (Note: All given as reduction) E° (V) 02 (g) + 4 H*(aq) + 4 e 2 H20 (1) 1.229 Z2 (s) + 2 e 3+ (aq) + 3 e 2z (aq) 0.426 A (s) 0.292 2 H20 (1) + 2 e G2+ (aq) + 2 e M²+ (aq) + 2 e¯ H2 (g) + 2 OH¯ (aq) - 0.828 G (s) - 1.245 M (s) - 1.893 A student constructs a voltaic electrochemical cell with two metal electrodes [metal G and metal A] in their respective aqueous nitrate solutions [G(NO3)2 and A(NO3)3]. Use this information, as well as the reduction potentials in the table above to complete each statement below. Consider the same cell from the above prompt. Calculate A E°. cell for this galvanic cell given the reference information given at the top of the quiz. Report your answer with 3 decimal places. You do not need to report units with your answer.
Calculate the equilibrium constant of the reaction Zn (k) + Fe²+ (aq) Fe (k) at 25 °C. E°(Zn²+ | Zn)= -0.76 V E°(Fe²+| Fe)= - 0.44 V ==> Zn²+(aq) +

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