Balance the half-reactions assuming that they occur in acidic
solution.Express your answer as a balanced half-reaction. Identify
all of the phases in your answer.
1) NO3−(aq)→NO(g)
2)Zn(s)→Zn2+(aq)
3)Te(s)→TeO2(s)
4)Sn4+(aq)→Sn2+(aq)
3. Balance the following redox reactions that occur in
acidic solution using the half-reaction method.
a. Cr(s) + NO3-(aq) → Cr3+(aq) + NO(g)
b. CH3OH(aq) + Ce4+(aq) → CO2(aq) +
Ce3+(aq)
c. SO32-(aq) + MnO4-(aq) → SO42-(aq) +
Mn2+(aq)
complete and balance the net ionic equations for reactions that
would occur:
Zn(s)+Mg2+(aq)--->
Zn(s)+Cu2+(aq)---->
Zn(s)+H+(aq)----->
Mg(s)+Zn2+(aq)----->
Mg(s)+Cu2+(aq)--->
Mg(s)+H+(aq)---->
Cu(s)+Zn2+(aq)---->
Cu(s)+Mg2+(aq)---->
Cu(s)+H+(aq)----->
The following two half-reactions occur in a standard alkaline
battery:
Zn(s) + 2OH-(aq) → ZnO(aq) + H2O(l) +
2e-
MnO2(s) + H2O(l) + e- →
MnO(OH)(s) + OH-(aq)
(a) Describe how the spontaneous flow of
electrons occurs in a simple battery (2 pts).
(b) Identify the cathode and anode of the
standard alkaline battery (2 pts).
(c) Identify the element that is oxidized
and the element that is reduced (2 pts).
(d) Identify the species that acts as the
oxidizing agent and the species...
Balance the following redox reaction in acidic solution by
adding the appropriate coefficients. H+(aq)+Mn2+(aq)+NaBiO3(s)
=> H2O(l) +MnO4(aq)+Br3+(aq)+Na+(aq). Show steps please.
Balance the following redox reaction in acidic solution by
adding the appropriate coefficients. H+(aq)+Mn2+(aq)+NaBiO3(s)
=> H2O(l) +MnO4(aq)+Br3+(aq)+Na+(aq). Show steps please.
the reaction 2 h2o2(aq) -> 2 h2o(l) + o2(g) is first order in
h2o2 and has a rate constant of 0.00785 s- at 24C. a reation vessel
contains 190ml of 25% h2o2 by mass solution (density of the
solution is 1.09 g/ml). the gaseous oxygen is collected over water
at 24Cas it forms. What volume of o2 forms in 146 seconds at a
barometric pressure of 747.9 mmHg?