1- Consider the reaction 2NHle) CO(e) o NH,CONHlag) H,O). Given that ?G\"--27.2
ID: 1045652 • Letter: 1
Question
1- Consider the reaction 2NHle) CO(e) o NH,CONHlag) H,O). Given that ?G"--27.2 Kj, calculate a) Calculate the equilibrium constant (Kc) for the above reaction at 25°C b) Calculate AG at 25 C when the concentrations are: [NH]-1.0M, [Co.] -10.0 M and [NH CONH2]-1.0M c) How would the temperature affect the spontaneity of the reaction with these concentrations? 2- State whether the sign of the entropy change expected for each of the following processes will be positive or negative, and explain your predictions a) 201g) ? 301g) b) 2CO)(g)2CO(8)Oe) c) 2NaHCOs(s) Na CO(s)COz(8) + HOU) 3- Balance the following redox equations a) NO+CIO2NO +CIO2 (in basic solution b) Br. + ????, cio2 + Br2 (in acidic solution) 4- Consider the Redox reaction where H,O(U) is oxidized to HyO-(aq), and COlg) is reduced to H2C204(aq). a) Balance the reduction reaction and balance the oxidation reaction b) Determine the standard cell potential (Ece), and the number of exchanged electrons (n) c) Calculate the equilibrium constant at 25 °C for the reaction How many grams of Platinum(Pt) will be obtained when an aqueous Pt(NO,) solution is electrolyzed for 30.00 min with a constant current of 3.40 A 5- 6- (10 extra points) Using Appendix B, calculate the Ksp of Copper(I)Phosphate.Explanation / Answer
1.
(a)
deltaG0 = - R T lnK
- 27.2 = - 0.008314 * 298.15 * lnK
lnK = 11.0
K = 58277
K = 5.83 * 104
(b)
Q = [NH2CONH2] / [NH3]2[CO2]
Q = 1.0 / (1.0)2(10.0)
Q = 0.10
deltaG = deltaG0 + R T lnQ
deltaG = - 27.2 + 0.008314 * 298.15 * ln(0.10)
deltaG = - 32.9 kJ
(c) Since entropy change of the reaction is negative, the reaction is spotaneous on the basis of exotehrmic nature of reaction. SO, increase in temperature will favour endothermic reaction i.e backward reaction in this case. Hence increase in temperature will decrease the spontaneity of the reaction.
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