swing the next reaction
Cr2O72-+I- ---> Cr3+I2
and write the coefficients
[ ] I-+ [ ]H++ [ ] Cr2O72- [ ] I2+[ ] H2O+[ ] Cr3+
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swing the next reaction Cr2O72-+I- ---> Cr3+I2 and write the coefficients [ ] I-+ [ ]H++...
Consider the reaction
Cr2O72−(aq) +
I−(aq)
→ Cr3+(aq) + I2(s).
In the reaction of dichromate ion and iodide ion: Cr2O72-(aq) + 14 H+(aq) + 6 I-(aq) ---> 2 Cr3+(aq) + 7 H2O(l)+ 3 I2 (s) the oxidizing agent is ? and the reducing agent is ?
In the redox reaction Cr2O72- (aq) + I1- (aq) ---> Cr3+ (aq) + I2 (s), what is the balanced oxidation reaction (before the half reactions are added together)?
Using the Nernst equation, calculate the cell potential for the following reaction (T=298 K): Cr2O72- (aq) + 14 H+ (aq) 6 I- (aq) → 2 Cr3+ (aq) + 3 I2 (s) + 7 H2O (l) given that Cr2O72- = 1.7 M H+ = 1 M I- = 1 M Cr3+ = 0.002 M
Balance the redox reaction by inserting the appropriate coefficients. redox reaction: H^+ + CrO2^−4 + NO−2⟶Cr3+ + H2O + NO^−3
Question 22 (4 points) Cr2O72- + 3 H2O2 + 8 H+ + 2 Cr3+ + 3 O2 + 7 H2O In the above reaction Ocrin Cr₂O7 2- is reduced. OH in H+ is oxidized. Cr₂O7 2 is the oxidizing agent and H2O2 is the reducing agent. Cr₂O7 2- is the reducing agent and H2O2 is the oxidizing agent.
Complete and balance the following half-reaction in basic solution Cr2O72-(aq) 2 Cr3+ (aq) 04- 03.02 + 2+ 3+ 4+ 1 3 4 5 N 6 7 8 9 0 12 n 4 Os 06 07 co 0, 0. + on (s) (1) (g) ((aq) O H2O ОН" H + CD H30+ С
Balance the redox reaction by inserting the appropriate coefficients. redox reaction: H+ + Cro- + NO3 + Cr3+ + H2O + NO3
Balance the following equations. (Use the lowest possible
whole-number coefficients. These may be zero.)
(a) MnO4-(aq) + Cl-(aq) Mn2+(aq) + Cl2(aq)
MnO4- + Cl-
+ H+ + H2O Mn2+
+ Cl2 + H+
+ H2O
(b) Cr2O72-(aq) +
NO2-(aq) Cr3+(aq) +
NO3-(aq)
Cr2O72-
+ NO2- + H+
+ H2O Cr3+
+ NO3- + H+
+ H2O
(c) Tl2O3(s) + NH2OH(aq) TlOH(s) + N2(g)
Tl2O3 + NH2OH
+ OH- + H2O TlOH(s) + N2
+ OH- + H2O
(d) CrO42-(aq) +
C2O42-(aq) Cr(OH)3(s) +
CO2(g)
CrO42-
+ C2O42-
+ OH- + H2O Cr(OH)3
+ CO2 + OH-
+ H2O
For the following reaction in acidic solution As2O3 + I2 → H3AsO4 + I- a correct set of stoichiometric coefficients in the balanced equation is As2O3 H2O I- A. 2,10,2 B. 1,5,2 C. 1,5,4 D. 1,10,2 E. 2,5,4