Hydrogen peroxide (H_2 O_2) decomposes according to the equation H_2 O_2 (I) rig

Question

Hydrogen peroxide (H_2 O_2) decomposes according to the equation H_2 O_2 (I) right arrow H_2O (I) + 1/2 O_2(g). Calculate K_p for this reaction at 25 de3gree C. (deltaH^o = -98.2 Kj/mol, deltaS^o = 70.1 J/k.mol) Complete and balance the following redox equation. What is the coefficient of OH when the equation is balanced using the set of smallest whole-number coefficients MnO_4 + SO_3^2- right arrow Mn^2+ + SO_4^2- (acidic solution) 3 4 5 8 none of these. Complete and balance the following redox equation. What is the coefficient of OH" w! the equal ion is balanced using the set ol smallest whole-number coefficient MnO_4^- + 1^- right arrow MnO_2 + IO_3^- (basic solution) 1 2 4 10 None of these. For the reaction, 2Cr^2+ + Cl_2(g) right arrow 2Cr^3+ + 2C1^-, E degree cell is 1.78 V. Calculate E degree cell related reaction Cr^3+ + Cl ^- Cr^2 + 1/2Cl_2(g).

Explanation / Answer

Solution :-

Q5) For the given reaction Delta H is negative and Delta S is positive

Therefore reaction is spontaneous at all temperatures.

So the correct answer is option B

Q6) formula to calculate the Delta G reaction is as follows

Delta G rxn = sum of delta G product – sum of delta G reactant

                     = [(HNO3*2)+(NO*1)] –[(NO2*3)+(H2O*1)]

                     =[(-79.9*2)+(86.7*1)] –[(51.8*3)+(-237.2*1)]

                    = 8.7 kJ

So the correct answer is option A

Q7) Delta H = -199 kJ per mol

Delta S= -4.1 J per mol K * 1 kJ / 1000 J = -0.0041 kJ per mol K

Using the delta H and delta S we can calculate the delta G

Delta G= Delta H – (T*delta S)

             = -199 kJ – (298 K * (-0.0041 kJ per mol K))

            = -198 kJ / mol

So the correct answer is option E.

Q8)` delta H =-98.2 kJ per mol

Delta S = 70.1 J per mol K * 1 kJ / 1000 J = 0.0701 kJ per mol K

Now lets calculate the delta G

Delta G= Delta H – (T*delta S)

             = -98.2 kJ per mol – ( 298 K * 0.0701 kJ per mol K)

             = -119.09 kJ /mol

Now using the delta G value lets calculate the Kp

Delta Go = - RT ln Kp

(-119.09 kJ per mol * 1000 J / 1 kJ) = - 8.314 J per mol K * 298 K * ln Kp

(-119.09 kJ per mol * 1000 J / 1 kJ) / - 8.314 J per mol K * 298 K = Kp

48.067 = ln Kp

Anti ln [48.067] = Kp

7.5*10^20 = Kp

So the correct answer is option D

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