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Calculate Eºcell for each of the following balanced redox reactions. O2(g) + 2H2O(1) + 4Ag(s) +...
In the reaction 2Ag, O(s) + 4Ag(s) + O2(g) 4.58 L of O2 was formed at P = 745mmHg and T = 308K. How many grams of Agdecomposed? Express the mass in grams to three significant figures. V AEON O ? mAg,0 = 3.56 Submit Previous Answers Request Answer X Incorrect; Try Again
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.
Exercise 19.65 Use tabulated half-cell potentials to calculate AG for each of the following reactions at 25 C. Part A Pb2+ (aq) +Mg(e)-Pb(a) +Mg (aq) VAZD AGn Submit Request Answer Part B Br ()+2Cl (aq)-+2Br (aq) + Cl( Express your answer using two significant figures AG Submit Request Answer Part C MnO2(a)+ 4H (aq) + Cu()Mn (ag) +2H,O( Express your answer using two significant figures
Calculate the equilibrium constant for each of the reactions at 25∘C. Standard Electrode Potentials at 25 ∘C Reduction Half-Reaction E∘(V) Fe3+(aq)+3e− →Fe(s) -0.036 Sn2+(aq)+2e− →Sn(s) -0.14 Ni2+(aq)+2e− →Ni(s) -0.23 O2(g)+2H2O(l)+4e− →4OH−(aq) 0.40 Br2(l)+2e− →2Br− 1.09 I2(s)+2e− →2I− 0.54 A) 2Fe3+(aq)+3Sn(s)→2Fe(s)+3Sn2+(aq) (answers are not 4.1x10^5, 3.3x10^3, 2.7x10^10, or 2.6x10^10) B) O2(g)+2H2O(l)+2Ni(s)→4OH−(aq)+2Ni2+(aq) C) Br2(l)+2I−(aq)→2Br−(aq)+I2(s) (answer is not 1.7x10^18)
calculate the equilibrium constants at 25∘C for each of the following reactions. 2 CO(g) + O2(g) = 2 CO2(g) Express your answer using two significant figures. IVO ALQ R o a ? K = Submit Request Answer Part B 2 H2S(9) = 2 H2(g) + S2(g) Express your answer using two significant figures. CO ALQ O ?
Calculate the equilibrium constant for each of the reactions at 25 °C. Part B You may want to reference (Pages 861 - 865) Section 19.5 while completing this problem. O2 (g) + 2H20 (1) + 2Cu (s) ~40H(aq) + 2Cu²+ (aq) Express your answer using two significant figures. EVO ALO ? K = Submit Previous Answers Request Answer Cr(s) + Fe2+ (aq) → Cr3+ (aq) + Fe(s) Express your answer as a chemical equation. Identify all of the phases in...
At 74.0 °C, what is the maximum value of the reaction quotient, Q, needed to produce a non-negative Ecell value for the reaction SO42- (aq) + 4H+ (aq) + 2Br - (aq) = Br2 (1) + SO2 (g) + 2H2O(1) In other words, what is Q when Ecell = () at this temperature? Express your answer numerically to two significant figures. View Available Hint(s) IVO ADD A O O ?
Exercise 18.67: Problems by Topic - Cell Potential, Free Energy, and the Equilibrium Constant Calculate the equilibrium constant for each of the reactions at 25 ∘C. Part A Pb2+(aq)+Mg(s)→Pb(s)+Mg2+(aq) Express your answer using one significant figure. K = 5×1075 SubmitMy AnswersGive Up All attempts used; correct answer displayed Part B Br2(l)+2Cl−(aq)→2Br−(aq)+Cl2(g) Express your answer using one significant figure. K = 6•10−10 SubmitMy AnswersGive Up Incorrect; Try Again; 5 attempts remaining Part C MnO2(s)+4H+(aq)+Cu(s)→Mn2+(aq)+2H2O(l)+Cu2+(aq) Express your answer using one significant figure....
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?
Question 22 (5 points) Given the following half reactions: PbO2 + 4H+ + SO42- + 2e → PbSO4(s) + 2H20 E° = 1.69V PbO2 + 4H+ + 2e- → Pb2+ + 2H2O E° = 1 .46V Calculate the Ksp for PbSO4 at 25 degrees C. Please enter your answer in scientific notation, such as 1.2E10 or 1.2E-10 and keep two significant figures.