Question

Consider the redox reaction 2VO4^3-(aq) + SO2(g) + 8H^+(aq)--->2VO^2+(aq)+SO4^2-(aq)+4H2O(L) the oxidizing agent is VO4^3-(aq), VO2^+(aq), H^+(aq),...

Consider the redox reaction

2VO4^3-(aq) + SO2(g) + 8H^+(aq)--->2VO^2+(aq)+SO4^2-(aq)+4H2O(L)

the oxidizing agent is VO4^3-(aq), VO2^+(aq), H^+(aq), SO2(g), SO4^2-(aq)

Science   Chemistry   
0 0
Add a commentTranscribed image text
Next >

Homework Answers

Answer #1

2VO4^3-(aq) + SO2(g) + 8H^+(aq)--->2VO^2+(aq)+SO4^2-(aq)+4H2O(L)

oxidizing agent = the one that is being reduced

agents are found in the "reactants" part so

2VO4^3-(aq) + SO2(g) + 8H^+(aq) must be the answer

SO2 --> S(+4)

SO4-2 --> S(+6)

S is losing 2 electrons, thereore it is being oxidized, this is the reducing agent

therefore

2VO4^-3 must be the oxidizing agent

makes sense, since it is losing oxigens, therefore it is giving Oxygen to oxidize other substances

0 0
Know the answer?
Your Answer:

Post as a guest

Your Name:

What's your source?

Earn Coins

Coins can be redeemed for fabulous gifts.

Log In

Sign Up

Not the answer you're looking for?
Ask your own homework help question
Similar Questions
Consider the following redox reaction: 5Fe2+(aq)+MnO−4(aq)+8H+(aq)→5Fe3+(aq)+Mn2+(aq)+4H2O(l) Part A - What is the oxidation state of iron...
Consider the following redox reaction: 5Fe2+(aq)+MnO−4(aq)+8H+(aq)→5Fe3+(aq)+Mn2+(aq)+4H2O(l) Part A - What is the oxidation state of iron before the reaction? Part B - What is the oxidation state of manganese before the reaction? Part C - What is the oxidation state of hydrogen before the reaction? Part D - What is the oxidation state of oxygen before the reaction? Part E - What is the oxidation state of iron after the reaction? Part F - What is the oxidation state of...
d. 2 H+(aq) + 2 CrO42-(aq) → Cr2O72-(aq) + H2O(l) Is this a redox reaction? (yes...
d. 2 H+(aq) + 2 CrO42-(aq) → Cr2O72-(aq) + H2O(l) Is this a redox reaction? (yes or no) _____________ If yes: i. what is the oxidizing agent? ___________________ ii. what is the reducing agent? ___________________ iii. what species is being oxidized? __________________ iv. what species is being reduced? __________________
Balance the following redox equation. Cu(s) + H+(aq) + SO42−(aq) → Cu2+(aq) + H2O(l) + SO2(g)
Balance the following redox equation. Cu(s) + H+(aq) + SO42−(aq) → Cu2+(aq) + H2O(l) + SO2(g)
Determine the oxidizing agent in the following reaction. Mg(s) + 2 HCl(aq) → MgCl2(aq) + H2(g)...
Determine the oxidizing agent in the following reaction. Mg(s) + 2 HCl(aq) → MgCl2(aq) + H2(g) A) Mg B) H C) Cl D) N/A I KNOW THE ANSWER IS H, BUT PLEASE EXPLAIN IN GREAT DETAIL HOW YOU KNOW AND HOW YOU GET TO THAT RESULT !!!!!!!!!
What is the oxidizing agent in the following reaction? H2C2O4(aq) + 2KMnO4(aq) + 6HCl → 2MnCl2(aq)...
What is the oxidizing agent in the following reaction? H2C2O4(aq) + 2KMnO4(aq) + 6HCl → 2MnCl2(aq) + 2KCl(aq) + 10CO2(g) + 8H2O(l)
Consider the following reaction CaSO4 (s) ------- Ca +2 (aq) + SO4 -2 (aq) A. Calculate...
Consider the following reaction CaSO4 (s) ------- Ca +2 (aq) + SO4 -2 (aq) A. Calculate delta H B. Calculate delta S C. Calculate delta G at 25 C
Balancing Redox Equations 2 Balance each of the following net ionic equations for a redox reaction....
Balancing Redox Equations 2 Balance each of the following net ionic equations for a redox reaction. Part A VO2+(aq)+H+(aq)+ClO2−(aq)→VO2+(aq)+ClO2(g))+H2O(l) Express your answer as a net ionic equation. Identify all of the phases in your answer. SubmitMy AnswersGive Up Part B SO32−(aq)+MnO4−(aq)+H+(aq)→SO42−(aq)+Mn2+(aq)+H2O(l) Express your answer as a net ionic equation. Identify all of the phases in your answer. SubmitMy AnswersGive Up Part C S2O32−(aq)+Cl2(g)+H2O(l)→SO42−(aq)+Cl−(aq)+H+(aq) Express your answer as a net ionic equation. Identify all of the phases in your answer.
Potassium permanganate, KMnO4, is a powerful oxidizing agent. The products of a given redox reaction with...
Potassium permanganate, KMnO4, is a powerful oxidizing agent. The products of a given redox reaction with the permanganate ion depend on the reaction conditions used. In basic solution, the following equation represents the reaction of this ion with a solution containing sodium sulfite: MnO4−(aq)+SO32−(aq)→MnO2(s)+SO42−(aq) Since this reaction takes place in basic solution, H2O(l) and OH−(aq) will be shown in the reaction. Places for these species are indicated by the blanks in the following restatement of the equation: MnO4−(aq)+SO32−(aq)+     −−−→MnO2(s)+SO42−(aq)+     −−− Part B...
Given the equilibrium reactions: #1) SO2(aq) + H2O(l) = HSO3- (aq) + H+(aq) #2) HSO3- (aq)...
Given the equilibrium reactions: #1) SO2(aq) + H2O(l) = HSO3- (aq) + H+(aq) #2) HSO3- (aq) + H+(aq) = SO32- + 2H+(aq) What is the equilibrium constant for reaction #1 if the concentration of SO2 is 8.50E-20 M, SO32- is 0.619 M, and H+ is 2.00E-07 M? You know that the equilibrium constant (K) for reaction #2 is 130.
Consider the following redox reaction: 3 NO2 + 3 H2O →2 NO3- + 2 H3O+ +...
Consider the following redox reaction: 3 NO2 + 3 H2O →2 NO3- + 2 H3O+ + NO. Which species gets oxidized? Which species gets reduced? Which species is the oxidizing agent? Which species is the reducing agent? Which species gains electrons? . Which species loses electrons?
ADVERTISEMENT
Need Online Homework Help?

Get Answers For Free
Most questions answered within 1 hours.

Ask a Question
ADVERTISEMENT