Question

Complete and balance this equation for a reaction in acidic medium using smallest whole #'s.

Reaction: As2O3 + NO-3----> H3AsO4 + NO (split into 1/2 reactions first)

Answer #1

Complete and balance the following redox equation using the
smallest whole number coefficients. What is the coefficient of I2
in the balanced equation?
MnO4-(aq) + I- --> Mn2+ + I2 (acidic solution)

Balance the following redox reaction in acidic solution using
the half-reaction method, with smallest whole-number
coefficients.
MnO4−(aq) + S2O32−(aq) → Mn2+(aq) + SO42−(aq)
_____ MnO4−(aq) + _____ S2O32−(aq) + _____ H+(aq) → _____
Mn2+(aq) + _____ SO42−(aq) + _____ H2O(l)

1) Balance the reaction Fe2+ + MnO4– → Fe3+ + Mn2+ in acidic
solution. What is the correct coefficient for Fe2+ when the
smallest whole number coefficients are used?
2) Balance the reaction Fe2+ + H2O2 → Fe3+ + H2O in acidic
solution. How many electrons are exchanged when the smallest whole
number coefficients are used?
3) Balance the reaction Cu + HNO3 → Cu2+ + NO in acidic
solution. What is the correct coefficient for NO when the smallest...

Balance the following reaction assuming acidic solution:
Fe(OH)2(s) + CrO42-(aq) -->
Fe2O3(s) +
Cr(OH)4-(aq)
balance the reaction with the smallest whole number
coefficient.

When the following redox equation is balanced with smallest
whole–number coefficients, the coefficient for
ReO41- will be _____.
Au(s) +
ReO4–(aq) --> Re(s)
+ Au3+(aq) (acidic solution)
A.
2
B.
3
C.
7
D.
8
E.
None of these choices is correct.

(a) Balance the following equation by entering the smallest
possible whole-number coefficients into the blank.
_____ Na2SO4(s) +
_____C(s) ---- _____ Na2S(s) + _____
CO(g)
(b) If you start with 49.6 g of sodium sulfate and 16.5 g
carbon, calculate the maximum mass of sodium sulfide that could be
produced.
_____ g
(c) Assume the reaction trial in part (b) has a 100% yield (or
completion rate). Calculate the mass of excess reactant that will
remain.
_____ g
(d) If...

Complete and balance the equation where Cl2 reacts with Ag+ in
an acidic solution to yield AgCl(s) and ClO3-.

Obtain the balanced equation, using the lowest possible whole
numbers, for the redox reaction in acidic solution:
CH3OH(aq) + Cr2O72−(aq)
→ CH2O(aq) + Cr3+(aq) How many H+
appear in the final balanced equation, and which side are they
on?
A) 8, reactant side
B) 8, product side
C) 14, reactant side
D) 6, product side
E) 12, reactant side
Answer is A. Please explain step by step.

Balance the following oxidation-reduction reactions, which occur
in acidic solution, using the half-reaction method. (Use the lowest
possible coefficients. Include states-of-matter under the given
conditions in your answer.) NO3−(aq) + Sn(s) → NO(g) + Sn2+(aq)

Consider the conproportionation reaction between MnO4–(aq) and
Mn2+(aq) leading to MnO2(s).
(a) Balance the conproportionation reaction in acidic media
using smallest whole number coefficients.
(b) Explain the meaning behind, “conproportionation.”
(c) Evaluate ∆Eo (V) for the conproportionation reaction in (a).
The standard reduction potential
between MnO4–(aq) and MnO2(s) is +1.68 V.
(d) Is this conproportionation reaction spontaneous? (Yes/No)
Explain your choice.

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