16.Which of the following is intermolecular redoxreaction :-СНОCH,OHOH(1) 2|СНОCOOH(2) 2C,H;CHOAl(OC,H5 )3CH,COOH + C,H,CH,OH(3) 4CrO, + 6H,SO,→ 2Cr, (SO,); + 6H,O + 70,(4) As,S; + HNO; → H;AsO, + H,SO, + NO

The reaction in which reduction as well oxidation reaction is called redox reaction. Redox reactions…

16. Which of the following is intermolecular redox reaction :- СНО CH,OH OH (1) 2| СНО СООН (2) 2C,H;CHO Al(OC,Hs )3 C,H,COOH + C,H,CH,OH (3) 4CrO, + 6H,SO, → 2Cr, (SO,); + 6H,O + 70, (4) As,S, + HNO; → H;AsO, + H,SO, + NO

16. Which of the following is intermolecular redox reaction :- СНО CH,OH OH (1) 2| СНО СООН (2) 2C,H;CHO Al(OC,Hs )3 C,H,COOH + C,H,CH,OH (3) 4CrO, + 6H,SO, → 2Cr, (SO,); + 6H,O + 70, (4) As,S, + HNO; → H;AsO, + H,SO, + NO

Chemistry by OpenStax (2015-05-04)

1st Edition

ISBN:9781938168390

Author:Klaus Theopold, Richard H Langley, Paul Flowers, William R. Robinson, Mark Blaser

Publisher:Klaus Theopold, Richard H Langley, Paul Flowers, William R. Robinson, Mark Blaser

Chapter16: Thermodynamics

Section: Chapter Questions

Problem 2E: What is a nonspontaneous reaction?

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What is a nonspontaneous reaction?
Actually, the carbon in CO2(g) is thermodynamically unstable with respect to the carbon in calcium carbonate(limestone). Verify this by determining the standardGibbs free energy change for the reaction of lime,CaO(s), with CO2(g) to make CaCO3(s).
What characterizes an electrolytic cell? What is an ampere? When the current applied to an electrolytic cell is multiplied by the time in seconds, what quantity is determined? How is this quantity converted to moles of electrons required? How are moles of electrons required converted to moles of metal plated out? What does plating mean? How do you predict the cathode and the anode half-reactions in an electrolytic cell? Why is the electrolysis of molten salts much easier to predict in terms of what occurs at the anode and cathode than the electrolysis of aqueous dissolved salts? What is overvoltage?
(a) Calculate the standard free-energy change and the equilibrium constant for the dimerization of NO, to N2O4 at 25°C (see Appendix D). (b) Calculate AG for this reaction at 25°C when the pres- sures of NO2 and N,O4 are each held at 0.010 atm. Which way will the reaction tend to proceed?
The autoionization of water at 25°C can be expressed as H,0(l) → H*(aq) + ОН (ад); Кw %3D 10-14 13. Using appropriate calculations, (a) Determine if this reaction is exothermic or endothermic. (b) Show whether this reaction will occur spontaneously. (c) Using the thermodynamics of the reaction, explain how Kw will change at temperatures (1) greater than 25°C and (2) less than 25°C. Species дн? (кJ/mol) AS: (J/K-mol) AG: (kJ/mol) H2O(g) H*(aq) оН ад) -241.8 188.71 -228.6 0.00 0.00 0.00 -230.0 -10.75 -157.2 H2O(1) -237.18 -285.8 69.91 O(aq) 249.17 160.95 231.75
The reaction Cr(NH3)6*(aq) + 3en(aq) --> Cr(en)3+*(aq) + 6 NH3(aq)where en represents ethylenediamine, is endothermic. What can possibly be true for the spontaneity of the reaction. the reaction is spontaneous for all temperatures. the reaction is spontaneous for low temperatures. the reaction is non-spontaneous for all temperatures. the reaction is spontaneous for high temperatures. not enough info to tell.
Predict whether the following reactions will be spontaneousin acidic solution under standard conditions:(a) oxidation of Sn to Sn2+ by I2 (to form I-), (b) reductionof Ni2+ to Ni by I- (to form I2), (c) reduction of Ce4+ to Ce3+by H2O2, (d) reduction of Cu2+ to Cu by Sn2+ (to form Sn4+).
Predict whether the following reactions will be spontaneous in acidic solution under standard conditions: (a) oxidation of Sn to Sn2+ by I2 (to form I -), (b) reduction of Ni 2+ to Ni by I - (to form I2), (c) reduction of Ce4+ to Ce3+ by H2O2, (d) reduction of Cu2+ to Cu by Sn2+ (to form Sn4+)
Calculate AH for the reaction, N2H4(1) + O2(g) -----> N2(g) + 2H2O(1), from the following data: 2NH3(g) = 3N20(g) -----> 4N2(g) + 3H2O(1) N20(g) = 3H2(g) 2NH3(g0 + 1/2O2(g) -----> N2H4(1) + H2O(1) H2(g) + 1/2O2(g) AH = -1010 KJ -----> N2H4(1) + H2O(1) AH = -317 KJ AH = -143 KJ %3D -----> H2O(1) AH = -286 KJ
(a) For 1.00 mol of H2O(1) at 25 °C, what Ap is required to obtain a AG of +1.000 kJ? The molar volume of H2O(I) is 18.02 cm /mol. (b) For exactly 1 mol of ideal gas at 25 °C and 1.00 atm, what Ap is necessary to obtain a AG of +1.000 kJ? (c) Explain the difference in the two Ap values that you calculated.
In nonaqueous solvents, it is possible to react HF to create H2F+. Which of these statements follows from this observation?(a) HF can act like a strong acid in nonaqueoussolvents, (b) HF can act like a base in nonaqueous solvents,(c) HF is thermodynamically unstable, (d) There is an acidin the nonaqueous medium that is a stronger acid than HF.
Ka of HNO2 in 25 degree is 4.5 x 10^-4. (a) Write the equilibrium chemical reaction corresponding to Ka for nitrous acid (HNO2) at 25°C. (b) Calculate ΔG° for the dissociation of nitrous acid in solution using the given Ka value. (c) What is the value of ΔG at equilibrium? (d) When [H+] = 5.0 × 10^-2 M, [NO2^-] = 6.0 × 10^-4 M, [HNO2] = 0.20 M, what is the value of ΔG?