Answer :-
A. Cd(s) + Al3+(aq) -------> Cd2+(aq) + Al(s)
This reaction does not occur because Cd is less reactive than Al.
Which reaction below does not occur upon mixing the O A reagents shown? Cd(s) + Al3+(aq)...
The reducing agent in the reaction below is 3CuCl2(aq)+2Al(s) →3Cu(s)+2AlCl3(aq) a. Al3+ b. Cu2+ c. Al d. Cu
given the following cell notation: Al(s)| Al3+(aq)|| Cd2+ (aq)| Cd(s) what is the overall (net) cell reaction?
Two standard reduction potentials are given below. Cd2+(aq) + 2 e− → Cd(s) E⁰red = −0.403 V Al3+(aq) + 3 e− → Al(s) E⁰red = −1.662 V There is only ONE submission for each part. (a) Which is a stronger reducing agent, Cd(s) or Al(s)? Cd(s) Al(s) (b) Which is the most difficult to oxidize, Cd(s) or Al(s)? Cd(s) Al(s) (c) Is Cd(s) able to reduce Al3+(aq) in a spontaneous reaction? is able is not able (d) Is Al(s) able...
please help, thanks!
7. What is the correct cell notation for the reaction below? Cd(aq)+Ni(s)-Cd(s)+ Ni(aq) a. Cd Cd| Ni | Ni d. Ni Cd I N | Ca b. Cd CdNi | Ni e. Cd |Cd Ni Ni 8. Calculate AS for the dissociation of dinitrogen tetraoxi de at 25°C NOdg) 2NO:(g) AG, J/mol)AH, J/mol) Substance NO) NOdg) +33.2 +51.3 +97.9 +9.2 d. +0.076 kJ K a.-2.10 kJ/K e +2.10kJ/K b. -0.550 kJ/K c.-0.208 kJ/K 9. Use the standard...
For a voltaic cell based on the reaction below, what reaction happens at the anode? 2Ni3+(aq)+Cd(s)→2Ni2+(s)+Cd2+(aq) Ni3+(aq)+e-→Ni2+(aq) Ni2+(aq)→ Ni3+(aq)+e- Cd2+(aq)+2e-→Cd(s) Cd(s)→Cd2+(aq)+2e- A student measures the voltage across different metal electrodes placed in a voltaic cell. Using a copper cathode, the voltages when using a first a tin, then gold anode are positive and negative, respectively. The order of chemical reactivity of the solid metals must be Au>Cu>Sn Au=Sn Sn>Cu>Au Au=Sn>Cu
4. Which of the following statements about the voltaic cell shown below is correct? Zn(s)[Zn** (aq)|| Cu** (aq)|Cu(s) (a) The oxidation half-reaction is clearly Zn(s) ® Zn** (aq) + 2 e. (b) The oxidation half-reaction is clearly Zn() Zn" (aq) +le. (C) The oxidation half-reaction could not be anything other than Cu(s) ® Cu (aq) +2 e. (d) It is obvious that the oxidation half-reaction is Zn(s) ® Cu(s). 5. Which of the following statements about the voltaic cell shown...
Consider the unbalanced chemical reaction shown below: Cu(s)+HNO3(aq)→Cu(NO3)2(aq)+NO(g)+H2O(l) The oxidation state of Cu in Cu(s)Cu(s) = The oxidation state of Cu in Cu(NO_3)_2(aq)Cu(NO3)2(aq) = The oxidation state of N in HNO_3(aq)HNO3(aq) = The oxidation state of N in NO(g)NO(g) = The total number of electrons transferred in this reaction is = The sum of the coefficients in the balanced chemical reaction =
1)Consider the following half-reactions: Half-reaction E° (V) Cl2(g) + 2e- > 2Cl-(aq) 1.360V Cd2+(aq) + 2e- > Cd(s) -0.403V Al3+(aq) + 3e- > Al(s) -1.660 The strongest oxidizing agent is: _______ enter formula The weakest oxidizing agent is: _______ The weakest reducing agent is: _______ The strongest reducing agent is: _______ Will Al3+(aq) reduce Cl2(g) to Cl-(aq)? _____yes or no Which species can be reduced by Cd(s)? If none, leave box blank. 2) Use the table 'Standard Reduction Potentials' located...
Be sure to answer all parts. Consider the following reaction: Cd(s) + Fe2+(aq) → Cd2+(aq) + Fe(s) E° (Fe2+ / Fe) =-0.4400 V, Eº (Cd2+ / Cd) = -0.4000 V Calculate the emf for this reaction at 298 K if [Fe2+] = 0.85 M and [Cd2+] = 0.010 M. E= Lv Will the reaction occur spontaneously at these conditions? o o yes no cannot predict o
Be sure to answer all parts. Consider the following reaction: Cd(s) + Fe2+(aq) → Cd2+(aq) + Fe(s) E o (Fe2+ / Fe) = −0.4400 V, E o (Cd2+ / Cd) = −0.4000 V Calculate the emf for this reaction at 298 K if [Fe2+] = 0.60 M and [Cd2+] = 0.010 M. E =____ V Will the reaction occur spontaneously at these conditions? yes no cannot predict