Calculate the standard potential for the reaction shown below at 25º?
Sn+4 (aq) + Cl – (aq) + 2 OH – (aq) ⟶ Sn+2 (aq) + ClO – (aq) + H2O (l)
Eº = Answer V
Calculate the standard potential for the reaction shown below at 25º? Sn+4 (aq) + Cl –...
Calculate the standard potential for the reaction shown below at 25º? 6 Hg+2 (aq) + 2 Cr (s) ⟶ 3 Hg2+2 (aq) + 2 Cr+3 (aq) Eº = Answer V
Question 8 (1 point) The standard potential of the cell Sn(s) Sn2(aq) || Cl(aq)| AgCl(s) | Ag(s) is +0,36 V at 25°C. If the standard reduction potential of the AgCl|Ag Cl-couple is 0.22 V, calculate the standard reduction potential of the Sn? Isn couple. 0 -0.14 V +0.36 V -0.07 V +0.14 V +0.58 V
Calculate the potential for the reaction below at 25ºC under the following conditions: [Fe+3 ]=0.0200M [Sn+2 ]=0.0200M [Fe+2 ]=1.50M [Sn+4 ]=1.50M 2 Fe+3(aq) + Sn+2 (aq) → 2 Fe+2 (aq) + Sn+4 (aq) E = Answer V
A chemist designs a galvanic cell that uses these two half-reactions: half-reaction standard reduction potential Cl 2 (g) + 2 e − → 2 Cl − (aq) = E 0 red + 1.359 V MnO − 4 (aq) + 2 H 2 O (l) + 3 e − → MnO 2 (s) + 4 OH − (aq) = E 0 red + 0.59 V cathode half reaction anode half reaction overall reaction cell potential at standard state
Calculate the standard potential, Eº, for this reaction from its AGⓇ value. X(s) + y4+ (aq) — X4+ (aq) + Y(s) AGⓇ = 74.0 kJ E = V
Calculate the potential for the reaction below at 25ºC under the following conditions: [Fe+3 ]=0.0200M [Sn+2 ]=0.0200M [Fe+2 ]=1.50M [Sn+4 ]=1.50M 2 Fe+3(aq) + Sn+2 (aq) → 2 Fe+2 (aq) + Sn+4 (aq)
the standard reduction potential is attached below Use the table of standard reduction potentials for the following exercises. 4. Predict the products of the following redox reactions, then identify which could spontaneously occur. a) H(aq) + Au (s) → b) H (aq) + Na (8) ► c) Au+ (aq) + Na (5) ► 5. Find a reagent that can oxidize Br" to Br2 but cannot oxidize CI'' to Cl? More than one reagent is possible, but you only need to...
1- For the following reaction, Na+(aq) + OH-(aq) + H+(aq) + Cl- (aq) à Na+(aq) + Cl- (aq) + H2O (l) Na+(aq) + Cl- (aq), ions not involved in the reaction, are called _________________ions. 2- For the following reaction, Na+(aq) + OH-(aq) + H+(aq) + Cl- (aq) à Na+(aq) + Cl- (aq) + H2O (l) What type of reaction is taking place? ____________________ 3- What is the mass in grams of 1.73 mol of MgBr2? __________ 4- What is the percentage composition...
Use the standard half-cell potentials listed below to calculate the standard cell potential for the following reaction occurring in an electrochemical cell at 25�C. (The equation is balanced.) Sn(s) + 2 Ag+(aq) ? Sn2+(aq) + 2 Ag(s) Sn2+(aq) + 2 e- ? Sn(s) E� = -0.14 V Ag+(aq) + e- ? Ag(s) E� = +0.80 V a)-1.08 V b)+1.74 V c)-1.74 V d)+0.94 V e)+1.08 V
u Calculate the standard cell potential for each reaction below, andnote whether the reaction is spontaneous under standard state conditions. 1. Mn(s)+Sn(NO3)2(aq)⟶Mn(NO3)2(aq)+Sn(s) 2. Na(s)+LiNO3(aq)⟶NaNO3(aq)+Li(s) ● 3. Mg(?)+Ni2+(??)⟶Mg2+(??)+Ni(?)