Ag (aq) CI (aq) 56.4 AgCl(s) S JK- mol-) AH f(kJ/mol) 72.68 96.2 Use the data given to calculate the value of AG° Ixn for the reaction at 25°C 105.58 F167.2 127.07 AGC1(s) Ag"(aq) +C1 (aq) O a. +32.5 kJ O b.+75.2 kJ O C. +55.7 kJ O d.-75.2 kJ O e. -55.7 kJ

Ag (aq) CI (aq) 56.4 AgCl(s) S JK- mol-) AH f(kJ/mol) 72.68 96.2 Use the data given to calculate the value of AG° Ixn for the reaction at 25°C 105.58 F167.2 127.07 AGC1(s) Ag"(aq) +C1 (aq) O a. +32.5 kJ O b.+75.2 kJ O C. +55.7 kJ O d.-75.2 kJ O e. -55.7 kJ

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

3.) Consider the reaction below. Reaction: AH°r (kJ/mole) 2 ICI (£) 17.78 L. (g) 247.551 l16.135 223.066 (/mole K) Which explains the outcome when 0.45 mol ½, 0.45 mol Cl2, and 2.42 mol ICl are added to a 2.0L flask at 25°C? A. [ICI] decreases B. [ICI] increases C. both [b] and [CL] increase D. at equilibrium Keywords: reaction quotient (Q), initial concentration(s), equilibrium concentration(s), equilibrium constant, forward reaction, reverse reaction, Q K. Q= K Concepts: Reaction Quotient, Chemical equilibrium
A critical reaction in the production of energy to do work or drive chemical reactions in biological systems is the hydrolysis of adenosine triphosphate, ATP, to adenosine diphosphate, ADP, as described by the reaction ATP(aq) + H,O(1) → ADP(aq) + HPO (aq) for which AGixn = -30.5 kJ/mol at 37.0 °C and pH 7.0. Calculate the value of AGxn in a biological cell in which [ATP] = 5.0 mM, [ADP] = 0.40 mM, and [HPO?-] = 5.0 mM. AGxn kJ/mol %3D Is the hydrolysis of ATP spontaneous under these conditions? O yes
asap plss thsnkassss dsadadawdafa
Consider the reaction 2NaOH(aq) + H2(g)—2Na(s) + 2H2O(l) for which AH° = 368.6 kJ and AS° = 15.30 J/K at 298.15 K. (1) Calculate the entropy change of the UNIVERSE when 1.759 moles of NaOH(aq) react under standard conditions at 298.15 K. ASuniverse= J/K (2) Is this reaction reactant or product favored under standard conditions? (3) If the reaction is product favored, is it enthalpy favored, entropy favored, or favored by both enthalpy and entropy? If the reaction is reactant favored, choose 'reactant favored'. Submit Answer
Please provide full
Given the information A+ B → 2D AH° = -682.0 kJ AS° = 296.0 J/K С — D ΔΗ. 392.0 kJ AS = -103.0 J/K calculate AG at 298 K for the reaction А +В — 2C -251.60 AG kJ Incorrect
Using the values in the table below, calculate AGxn at 375 K for the reaction: 3 CO g) + 4 NH3(g) → 3 CH3OH(g) + 2 N2(g) AH°F, kJ/mol AG°, kJ/mol S°, J/mol K COg) CH3OH(g) CH3OH NH3(aq) NH3(g) N2(9) -111 -137 198 -201 -162 238 -239 -166 127 -80 -27 111 -46 -17 193 192 +55 +15 -7 +100,414 +150
Given the information AS = 302.0 J/K AS = -153.0 J/K А +В — 2D AH = 699.7 kJ С — D AH' = 398.0 kJ calculate AG at 298 K for the reaction A +B → 20 AG" = kJ
O-234 kJ 234 kJ -150. kJ -117 kJ Given: -1835kJ AH°, AHᵒf (kJ/mol) -941 -840 QUESTION 12 Use the standard reaction enthalpies given below to determine AH°rxn for the following reaction: P4(g) + 10 Cl₂(g) → 4 PC|5(s) PC15(s) → PC13(g) + Cl₂(g) P4(g) + 6 Cl₂(g) → 4 PCl3(g) rxn IF7(g) IF 5(9) 2(g) 62.42 = ? ΔΗ° rxn AH°rxn = +157 kJ = -1207 KJ QUESTION 13 Use the AH°f and AH°rxn information provided to calculate AH°f for IF: IF7(9) + 12(g) → IF5(g) + 2 IF(g) AH°rxn = -89 kJ
Which of the following reactions proceeds with syn stereochemistry.
A chemical engineer is studying the two reactions shown in the table below. In each case, he fills a reaction vessel with some mixture of the reactants and products at a constant temperature of 136.0 °C and constant total pressure. Then, he measures the reaction enthalpy AH and reaction entropy AS of the first reaction, and the reaction enthalpy AH and reaction free energy AG of the second reaction. The results of his measurements are shown in the table. Complete the table. That is, calculate AG for the first reaction and AS for the second. (Round your answer to zero decimal places.) Then, decide whether, under the conditions the engineer has set up, the reaction is spontaneous, the reverse reaction is spontaneous, or neither forward nor reverse reaction is spontaneous because the system is at equilibrium. AH = -2220, kJ J AS = -5426. K C,H, (g) + 50,(8) → 3C0,g) + 4H,0() AG = kJ Which is spontaneous? O this reaction O the reverse reaction O neither ΔΗ 50. ky AS = 6CI, (g) + 2Fe,0.(s)…
For the reaction C(s,graphite) + 02(g) CO2(g) AG° = -394.3 kJ and AS° = 2.9 J/K at 290 K and 1 atm. This reaction is (reactant, product) favored under standard conditions at 290 K. The standard enthalpy change for the reaction of 2.38 moles of C(s,graphite) at this temperature would be kJ.