Determine whether or not the reaction indicated will occur spontaneously. 2Cu+(aq) + Ni(s) Ú 2Cu(s) + Ni2+(aq)
The Given Reaction:
Half cell Reaction:
Here,
valve is +ve, hence the cell will be feasible and Ni will displace
copper from its salt solution. In other words Nickel will reduce
Copper.
And
If
valve is +ve the the valve of
will be negative, we can say that the reaction will occur
spontaneously.
Determine whether or not the reaction indicated will occur spontaneously. 2Cu+(aq) + Ni(s) Ú 2Cu(s) +...
Predict whether the following reactions would occur spontaneously in aqueous solution at 25 °C. Assume that the initial concentrations of dissolved species are all 1.0 M Predict whether the following reactions would occur spontaneously in aqueous solution at 25 °C. Assume that the initial concentrations of dissolved species are all 1.0 M Predict whether the following reactions would occur spontaneously in aqueous solution at 25 °C. Assume that the initial concentrations of dissolved species are all 1.0 M Predict whether...
Step 1: Determine whether or not each redox reaction occurs
spontaneously in the forward direction using only the relative
postion of the half reactions on table 18.1. (No numbers in this
step.)
Step 2: Then, calculate the voltage of each of the
reactions.
(a) Ca2+(aq) + Zn(s)
Ca(s) + Zn2+(aq)
(b) 2Ag+(aq) + Ni(s)
2Ag(s) + Ni2+(aq)
(c) Fe(s) + Mn2+
Fe2+(aq) Mn(s)
Write the products for all the reactions below that are expected to occur spontaneously. If there isn't a reaction, write NR Cl2 (g) + 2I (aq) -> H2 (g) + F2 (g) -> Ni (s) + Cu2+ (aq) -> Fe (s) + Ni2+ (aq) -> Cu2+ (aq) + Ag (s) -->
15. Predict whether each reaction will occur spontaneously or not. If it does occur, write a balanced equation. a) Mg(s) + ZnCl2(aq) → b) Cu(s) + AlBr3(aq) → c) Al(s) + CuCl(aq) →
5) Will this reaction occur spontaneously as written? (3 points) why 3Pb(s) + NO3 (aq) + 8H(aq) 3Pb2+(aq) + 2NO(g) + 4H2O(1)
Using the table of standard reduction potentials, answer True or False. The reaction: 2Cu(s) + 2H+(aq) ⇋ 2Cu+(aq) + H2 (g) will occur (is spontaneous) at STP.
1. Calculate the value of E° for the reaction below; Pb2+ (aq) + Ni (s) → Ni2+(aq) + Pb (s) 2. Calculate the value of ΔG° for the reaction below using your value from Question one; Pb2+ (aq) + Ni (s) → Ni2+(aq) + Pb (s) 3. Balance the following redox reaction in acidic conditions; KMnO4 (aq) + NO (g) → MnO2 (s) + NO2(g)
A galvanic cell Zn | Zn?* || Ni? Ni runs spontaneously. If a current is imposed to turn this into an electrolytic cell, which of the following will occur? A) Zn(s) still gets oxidized at the same rate B) Zn(s) gets oxidized at a faster rate C) Nigets oxidized D) Ni2+ gets reduced E) Zn2+ gets reduced
A galvanic cell ZnZn? || Ni? Ni runs spontaneously. If a current is imposed to turn this into an electrolytic cell, which of the following will occur? A) Zn(s) still gets oxidized at the same rate B) Zn(s) gets oxidized at a faster rate C) Ni2gets oxidized D) Ni2+ gets reduced E) Zn2+ gets reduced
17. Write the overall cell reaction for the following voltaic cell. Cd(s)|Cd2+(aq)||Ni2+ (aq)|Ni(s) 18. Calculate the standard cell potential of the following cell at 25°C. Cd(s) Cd2+ (aq)||Ni2+ (aq) Ni(s)