calculate ΔE° of this equation ( and state spontaneous or not at standard conditions)
Cl2(g) + 2Br- → Br2 + 2cl-
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calculate ΔE° of this equation ( and state spontaneous or not at standard conditions) Cl2(g) +...
1. Which of the following reactions would be spontaneous at standard state conditions and 25C? EXPLAIN your answer. a. Cu2+ + 2Br- ---> Br2(aq) + Cu b. Br2(aq) + 2Cl- ---> Cl2(aq) + 2Br- c. Fe + Cu2+ ---> Fe2+ + Cu 2. What would happen to the cell potential for the reaction below if the concentration of Cr3+ were reduced to .010M? Explain your answer and show your work. 2Cr + 3Cu2+ ---> 2Cr3+ + 3Cu a. It would...
Which one of the following reactions is spontaneous (in the direction given) under standard elecrochemical conditions? A. Pb2+ + 2I- --> Pb + I2 B. Cu2+ + Fe ---> Cu + Fe2+ C. 2Au + Pt2+ --> 2Au+ + Pt D. Mg2+ + 2Br- --> Mg + Br2 E. 2Hg + 2Cl- +2H+ --> Hg2Cl2 + H2
2. Calculate the standard cell emf (cell potential) for electrochemical cells having the following overall cell reactions and predict if they are spontaneous: a) Sn(s) + Pb2+ (aq) → Sn?" (aq) + Pb(s) Eºcell = Volts. Spontaneous? b) 2002 (aq) + Zn?"(aq) → 2Co3+ (aq) + Zn(s) Eºcell__volts; Spontaneous? c) Cl2(g) + 2Br (aq) + 2Cl(aq) + Br2(1); E° = volts; Spontaneous?
Calculate the standard cell potential and determind deltaG for a cell that utilizes the following reaction: Cl2(g) + 2Br-(aq) -----> 2Cl-(aq) + Br2 (l)
Calculate DH for the reaction BrCl(g) -----> Br(g) + Cl(g) Given Br2(l) -----> Br2(g) DH = 30.91 kJ Br2(g) -----> 2Br(g) DH = 192.9 kJ Cl2(g) ------> 2Cl(g) DH = 243.4 kJ Br2(l) + Cl2(g) ----> 2BrCl(g) DH = 29.2 kJ
Calculate the equilibrium constant for each of the reactions at 25 ∘C. Standard Electrode Potentials at 25 ∘C Reduction Half-Reaction E∘(V) Pb2+(aq)+2e− →Pb(s) -0.13 Zn2+(aq)+2e− →Zn(s) -0.76 Br2(l)+2e− →2Br−(aq) 1.09 Cl2(g)+2e− →2Cl−(aq) 1.36 MnO2(s)+4H+(aq)+2e− →Mn2+(aq)+2H2O(l) 1.21 Pb2+(aq)+2e− →Pb(s) -0.13 Br2(l)+2Cl−(aq)→2Br−(aq)+Cl2(g) Express your answer using two significant figures.
Calculate the equilibrium constant K for the reactions at 298 K. a) Br2(g) + 2Cl-(aq) ---> 2Br-(aq) + Cl2(g) b) A Galvanic Cell with the SHE and Fe+2/Fe(s)
Under what conditions will the following reaction be spontaneous? SO2(g) + Cl2(g) → SO2Cl2(g) The following information may be important: ΔHºf SO2(g) = -296.8 kJ/mol, ΔHºf SO2Cl2(g) = 364.0 kJ/mol low temperatures high temperatures always spontaneous never spontaneous
An ionic compound, MBr, has ΔE for (M+1/2Br2 => MBr) = -500 kJ/mol. Given the information below, calculate its lattice energy. M(s) => M(g) ΔE = +140 kJ/mol M(g) => M+(g) + 1 e- ΔE = +500 kJ/mol Br2(l) => 2Br(g) ΔE = +200 kJ/mol Br(g) + 1 e- => Br-(g) ΔE = -325 kJ IE1 of Br(g) = +1143 kJ/mol
Question 5 (1 point) For the cell diagram Pt(s) | Br2(1) | Br"(aq) || C1-(aq)| Cl2(g) | Pt(s) which reaction occurs at the cathode? O 2C1-(aq) --> Cl2(g) + 2e- O 2Br (aq) --> Br2(1) + 2e O Br2(l) +2e --> 2Br (aq) O Cl2(g) + 2Br (aq) --> 2C1-(aq) + Br2(1) O C12(g) + 22 --> 2C1“(aq)