16A.3 Flashcards
in an electrochemical cell how does electrons flow
from the half cell with the more negative E, to the have cell with the more positive E
electrode potential can tell us
how easily a species loses electrons
what is a thermodynamically feasible reaction
a reaction that should take place without any intervention from us, if we consider the enthalpy and entropy changes involved
how is a reaction in electrochemical cell thermodynamically feasible
if there is a large gap between the standard electrode potential values with the element giving the electron having a more negative number
is the reaction between cupper (s) and dilute sulfuric acid and its reverse reaction thermodynamically feasible
no since cupper E is more positive so it wont give electrons to H, but the reverse reaction works but H gas is never bubbled into a cupper ion solution since too high Ea so the reactants are kinetically stable
what is a kinetically stable
the reaction does not take place, or is very slow, because the Ea of the reaction is very high
is the reaction between cupper and zinc thermodynamically feasible
yes since zinc has a more negative E
is the reaction between zinc and dilute sulfuric acid thermodynamically feasible
yes since zinc has a more negative E
What is the reaction between Manganese (IV) oxide and hydrochloric acid
MnO2 (s) + 4HCl(aq) ——> Mn^2+(aq) + 2Cl^-(aq) + 2H2O(l) + Cl2(g) (this is wrong lol)
is the reaction between Manganese (IV) oxide and hydrochloric acid thermodynamically feasible
no since Cl needs to release electrons but Mn is has a more negative E
What are the two have equations involved in Manganese (IV) oxide and hydrochloric acid
MnO2(s) +4H^+(aq) +2e- ——> Mn^2+(aq) + 2H2O(aq)
Cl2(g) + 2e- —-> 2Cl^-(aq)
how do we make the reaction between Manganese (IV) oxide and hydrochloric acid thermodynamically feasible
By increasing the concentration of hydrochloric acid to 10 mol dm^-3, that means that with more hydrogen ions the eq at MnO2 half cell will shift to the right and with more Cl ions the eq at Cl2 will shift to the left, so the E of MnO2 because more positive than the E of Cl2 allowing Cl to lose electrons and give to MnO2
the thermodynamic feasibility of a chemical reaction can be predicted using
standard electrode potential
the E values may indicate that a reaction is thermodynamically feasible yet it may not take place, what are the two reasons
- the reaction is kinetically stable because the Ea for the reaction is too large
- the reactions might not take place under standard conditions
a reaction might not be thermodynamically feasible under standard conditions but
may become feasible when the conditions are altered