Question

7) At 1500°C the equilibrium constant for the reaction CO(g) + 2H2(g) → 키.4x10-7. Calculate AG)for this reaction at 1500°C A) 105 kJ/mol B)-105 kJmol C)1.07 kJ/molD) CH,011(g) has the value K, D)255 8) Determine the equilibriurn constant K, at 25°C for the reaction Nag) + 3H2(g) → 2NHO 3 kJ/mol A) 1.52 x 106 B) 6.60 x 10 9) Predict the sign of AS for the reaction 02(g) → 20(g). C) 828 x 10D) 2.60 A) Negative B) zero (no sign) C) positive 10) Complete and balance the following redox equation that occurs in acidic solution using the set of smallest whole-number coefficients. What is the coefficient of H:0 in the equation? PbO2(s) + Cl-→ Pb2+ + Cl2(g) (acidic solution) A) 2 C) 5 D) 9 11) Given the following notation for an electrochemical cell Pt(s) H2(g) | H (aq) Il Ag (aq) | Ag(s) what is the balanced overall (net) cell reaction? A) 2H+(aq) + 2Ag+(aq) → H2(g) + 2Ag(s) B) Ha(g) + 2Ag(s) → H+(aq) + 2Ag+(aq) C) 2H+(aq) + 2Ag(s)--H2(g) + 2AgTaq) D) H2(g) + 2Ag(aq) → 2H"(aq) + 2Ag(s) 12) What is the oxidation number of Cr in Cro +6 D) +12 A) +2 B) +7 13) Consider an electrochemical cell constructed from the following half cells, linked by an exters circuit and by a KCl salt bridge. - an Al(s) electrode in 1.0 M AI(NO3)s solution - a Pb(s) electrode in 1.0 M Pb(NOs)2 solution The balanced overall (net) cell reaction is A) Pb(s) + Ap-(aq) → Pb?Taq) + Al(s). B) 3 Pb(s) + 2APTaq) → 3 Ps*(aq) + 2Al(s). C) 3Pb2"(aq) + 2Al(s) → 3Pb(s) + 2A13+(aq). D) Pb2+(aq) + Al(s) → Pb(s) + Ap-(aq). 14) A certain electrochemical cell has for its cell reaction: Zn +HgO-ZnO+ Hg Which is the half-reaction occurring at the anode? A) HgO + 2e-→Hg + 02- B) Zn2+ +2e-→Zn C) D) Zn→Zn2+ + 2e- ZnO + 2e-→Zn

Answer 1

23632.5 J/m& +232-632 ms

ろ Ice; 6.6x105