1. A piece of zinc metal is added to an acidic, yellow aqueous solution of vanadate...

1. A piece of zinc metal is added to an acidic, yellow aqueous solution of vanadate ion, dioxidovanadate(V), [VO₂]⁺. The solution turns blue due to formation of vanadyl ion, oxidovanadate(IV), [VO]²⁺.

Write a balanced equation for the oxidation half-reaction. (2 points)

Write a balanced equation for the reduction half-reaction. (2 points)

Solutions

Expert Solution

Reduction take place at vanadate ion as it converted from oxidation state 5 to oxidation state 4.

queen_honey_blossom answered 1 year ago

Next > < Previous

Related Solutions

-- A 1.0000 g sample of zinc metal is added to a solution containing 1.2500 g of...

-- A 1.0000 g sample of zinc metal is added to a solution containing 1.2500 g of an unknown compound of bismuth and chlorine. The reaction results in the formation of zinc chloride and metallic bismuth. When the reaction is complete, unreacted zinc remains, and this unreacted zinc is consumed by reaction with HCl. After washing and drying, the mass of bismuth metal recovered is 0.6763g. Q. Write a balanced chemical equation for the reaction of zinc with the original unknown...

Q.-- A 1.0000 g sample of zinc metal is added to a solution containing 1.2500 g...

Q.-- A 1.0000 g sample of zinc metal is added to a solution containing 1.2500 g of an unknown compound of bismuth and chlorine. The reaction results in the formation of zinc chloride and metallic bismuth. When the reaction is complete, unreacted zinc remains, and this unreacted zinc is consumed by reaction with HCl. After washing and drying, the mass of bismuth metal recovered is 0.6763g -- Calculate the experimental % of bismuth in the original unknown compound -- If...

When an aqueous solution of 7.00 g of BaCl2 was added to an aqueous solution of...

When an aqueous solution of 7.00 g of BaCl2 was added to an aqueous solution of 5.25 g of K2SO4, a white precipitate formed. After filtering and drying the precipitate, 6.85 g of BaSO4 powder was obtained. BaCl2 (aq) + K2SO4(aq) BaSO4(s) + 2 KCl (aq) What is the theoretical yield of BaSO4? SHOW ALL WORK. What is the percent yield of BaSO4? SHOW ALL WORK In determining the concentration of a sulfuric acid solution, 32.63 mL of a 0.100...

7. A piece of zinc metal with a mass of 35.0 g is heated in boiling...

7. A piece of zinc metal with a mass of 35.0 g is heated in boiling water to 101.3 ºC and then dropped into a coffee-cup calorimeter containing 75.0 g of water at 23.8 ºC. When thermal equilibrium is reached, the final temperature is 27.0 ºC. Calculate the specific heat capacity of the zinc.

When an aqueous solution of strontium chloride is added to an aqueous solution of potassium sulfate,...

When an aqueous solution of strontium chloride is added to an aqueous solution of potassium sulfate, a precipitation reaction occurs. Write the balanced net ionic equation of the reaction.

An aqueous solution containing 7.22g of lead (II ) nitrate is added to an aqueous solution...

An aqueous solution containing 7.22g of lead (II ) nitrate is added to an aqueous solution containing 6.02g of potassium chloride. Enter the balanced chemical equation for this reaction. Be sure to include all physical states.What is the limiting reactant?The % yield for the reaction is 84.1%, how many grams of precipitate were recovered? How many grams of the excess reactant remain?

When magnesium metal and an aqueous solution of hydrochloric acid combine, they produce an aqueous solution...

When magnesium metal and an aqueous solution of hydrochloric acid combine, they produce an aqueous solution of magnesium chloride and hydrogen gas. Using the equation, Mg (s) + 2HCl (aq) → MgCl2 (aq) + H2 (g), if 24.3 g of Mg and 75.0 g of HCl are allowed to react, calculate the mass of MgCl2 that is produced

If aluminum hydroxide is added to an acidic solution with a pH of 1.93, what is...

If aluminum hydroxide is added to an acidic solution with a pH of 1.93, what is the new pH after equilibrium is established? This problem is a bit tricky. So, extra help is given. The following ICE Table is useful: ... Al(OH)3(s) ↔ Al3+(aq) + 3OH-(aq) Ksp = 2.0 x10-32 M4 I: ...Excess ... ...0 ......... ...from pH C:.....-s....... ......s ...... ........3s E:...Excess ... ...s.......... .... ? (can't add) Hint, hydroxide produced neutralizes acid. [H+] =[H+]o -3s for 3s <...

An aqueous solution containing 6.36 g of lead(II) nitrate is added to an aqueous solution containing...

An aqueous solution containing 6.36 g of lead(II) nitrate is added to an aqueous solution containing 5.85 g of potassium chloride. Enter the balanced chemical equation for this reaction. Be sure to include all physical states. What is the limiting reactant? The percent yield for the reaction is 87.2%, how many grams of precipitate were recovered? How many grams of the excess reactant remain?

An aqueous solution containing 5.99 g of lead(II) nitrate is added to an aqueous solution containing...

An aqueous solution containing 5.99 g of lead(II) nitrate is added to an aqueous solution containing 5.04 g of potassium chloride. Enter the balanced chemical equation for this reaction. Be sure to include all physical states. balanced chemical equation: Pb(NO3)2(aq)+2KCl(aq)⟶PbCl2(s)+2KNO3(aq)Pb(NO3)2(aq)+2KCl(aq)⟶PbCl2(s)+2KNO3(aq) What is the limiting reactant? The percent yield for the reaction is 83.2%. How many grams of the precipitate are formed? How many grams of the excess reactant remain?

Subjects