(a)
Interpretation:
The oxidation states to all the elements in the given reaction should be assigned along with identify the reactant which is oxidized and reduced and also identify the oxidizing agent and reducing agent in the given reaction.
Concept Introduction :
A redox reaction is a
Oxidation state or oxidation number of an atom is defined as the positive or the negative charge that an atom would possess if it is present as ions in the given compound. In such type of reaction, the oxidation state of the atom undergoing oxidation will increase which depends upon the number of electrons lost by a particular atom.
Reduction of a chemical species refers to the gain of electrons by the chemical species which results in decrease in oxidation state of that atom.
A reducing agent is one which loses its electrons for the reduction of other chemical species which are undergoing redox reactions. In other words we can say that a reducing agent in a chemical reaction is the species which itself gets oxidized by loss of its electrons.
On the other hand an oxidizing agent is a chemical species which has the ability to oxidize other substances which are present in a chemical reaction. It acts by gaining electrons in a chemical reaction, thus itself gets reduced.
(b)
Interpretation:
The oxidation states to all the elements in the given reaction should be assigned and identify the reactant which is oxidized and reduced and also identify the oxidizing agent and reducing agent in the given reaction.
Concept Introduction :
A redox reaction is a chemical reaction in which oxidation and reduction reactions takes place simultaneously. In such type of reaction one of the chemical species is getting oxidized while the other species gets reduced at the same time.
Oxidation state or oxidation number of an atom is defined as the positive or the negative charge that an atom would possess if it is present as ions in the given compound. In such type of reaction, the oxidation state of the atom undergoing oxidation will increase which depends upon the number of electrons lost by a particular atom.
Reduction of a chemical species refers to the gain of electrons by the chemical species which results in decrease in oxidation state of that atom.
A reducing agent is one which loses its electrons for the reduction of other chemical species which are undergoing redox reactions. In other words we can say that a reducing agent in a chemical reaction is the species which itself gets oxidized by loss of its electrons.
On the other hand an oxidizing agent is a chemical species which has the ability to oxidize other substances which are present in a chemical reaction. It acts by gaining electrons in a chemical reaction, thus itself gets reduced.
(c)
Interpretation:
The oxidation states to all the elements in the given reaction should be assigned and identify the reactant which is oxidized and reduced and also identify the oxidizing agent and reducing agent in the given reaction.
Concept Introduction :
A redox reaction is a chemical reaction in which oxidation and reduction reactions takes place simultaneously. In such type of reaction one of the chemical species is getting oxidized while the other species gets reduced at the same time.
Oxidation state or oxidation number of an atom is defined as the positive or the negative charge that an atom would possess if it is present as ions in the given compound. In such type of reaction, the oxidation state of the atom undergoing oxidation will increase which depends upon the number of electrons lost by a particular atom.
Reduction of a chemical species refers to the gain of electrons by the chemical species which results in decrease in oxidation state of that atom.
A reducing agent is one which loses its electrons for the reduction of other chemical species which are undergoing redox reactions. In other words we can say that a reducing agent in a chemical reaction is the species which itself gets oxidized by loss of its electrons.
On the other hand an oxidizing agent is a chemical species which has the ability to oxidize other substances which are present in a chemical reaction. It acts by gaining electrons in a chemical reaction, thus itself gets reduced.
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Chapter 15 Solutions
Basic Chemistry
- (7.12) A technician plates a faucet with 0.86 g Cr metal by electrolysis of aqueous Cr2(SO4)3. If 12.5 min is allowed for the plating, what current is needed? Molar mass of Cr: 51.996 g/mol Analysis/Strategy: mass of Cr ® mol Cr mol e¯ (or Faraday) ® coulombs ® amperes Reduction half-reaction of chromium solution to chromium metal: Cr* ,+3, (aq) e¯ ® Cr(s) + chromium solution, Cr2(SO4)3, has the ions: [Cr*3 s04-²] Answer: The current needed is ampere. (2 sig fig)arrow_forwardFill in the blanks: (7.14) In the electrolysis of CUSO4, how much copper is plated out on the cathode by a current of a 0.75A in 10 minutes? (Cu 63.546 g/mol) Analysis/Strategy: ampere & time coulombs ® mol e¯ (or Faraday) ® mol Cu (R mass of Cu Reduction half-reaction of copper solution to copper metal: Cu*²(aq) + e¯ ® Cu(s) copper solution, CUSO4, has the ions: [Cu*2 SOq] Answer: The mass of copper plated out is g Cu. (3 sig fig)arrow_forward(7.1a) Complete and balance the following by ion-electron method. Reactions are taking place in acidic solution. a) Cu(s) + NO3 (aq) - Cu*taq) + NO2(g Analysis: Oxidation-Half reation: Balancing atoms & charges: Cu(s) Cu(aq) * e Reduction-Half reation: Balancing 0 & H and charges: H* + NO3 (aq) + e - NO2(g) H20 Balancing electrons lost & gained and balancing the equation: Cus) NO3 (aq) * H* - Cu(aq) NO2(g) H20arrow_forward
- For each of the reaction below, identify: (0.5 marks each) substance being oxidized substance being reduced oxidizing agent reducing agent number of electrons transferred. 1. K2Cr207 + 14HCI -> 2KCI + 2CrCl + 3Cl + 7H20 2. 10 OH +4C12 + S2032 > 5H20 + 2502 + 8 CIarrow_forwardFill in the blanks: (7.13) Using a current of 4.75 A, how many minutes does it take to plate a sculpture with 1.50 g of Cu from a CuS04 solution? (Cu 63.546 g/mol) Analysis/Strategy: mass of Cu ® mol Cu ® mol e" (or Faraday) ® coulombs ® time in minutes (given current in amperes) Reduction half-reaction of copper solution to copper metal: Cu*2(aq) · + e¯ ® Cu(s) copper solution, CUSO4, has the ions: [Cu*2_SOq] Answer: The time needed to plate out a sculpture is minutes. (3 sig fig)arrow_forwardComplete the following equations by writing the formula(s) of the product(s) and balancing the equation with coefficients. Use the type of reaction to aid in determining the products. 6. 7. 8. 9. Balanced Equation 10. Zn + FeCl3 + 12. C3H8 + HgO→ 13. Al + H₂SO4 → AgNO3 → 0₂ Cl₂ → Balanced Equation 11. Iron and oxygen react to form iron (III) oxide. afe +302 afe 203 Type of Reaction Single Replacement Write the balanced chemical equation for the following chemical reactions. Include the correct formulas for all reactants and products and balance with coefficients. Identify the type of reaction in the right column. Double Replacement Combustions Decomposition Combination Silver nitrate and magnesium chloride react to form magnesium nitrate and silver chloride. 2Aguo3 + MgCl₂ → 2 Agcl + ing [Nosta double displacement Type of Reaction Compustion Aluminum reacts with copper (II) sulfate to form aluminum sulfate and copper solid. 3 cu 50₂ +2A1-3 Cu +3504 +2A¹a (564)3 single displacment 10arrow_forward
- 8.10 Balance each of the following chemical equations: a. HNO3(aq) + Zn(s) → H₂(g) + Zn(NO3)2(aq) b. H₂SO4(aq) + Al(s) → H₂(g) + Al2(SO4)3(aq) c. K₂SO4(aq) + BaCl₂(aq) →→→ BaSO4(s) + KCl(aq) d. CaCO3(s) → CaO(s) + CO2(g) e. AlCl3(aq) + KOH(aq) → Al(OH)3(s) + KCl(aq)arrow_forward(7.1b) Complete and balance the following by ion-electron method. Reactions are taking place in acidic solution. b) Mn*2(aq) + BiO3 (aq) Bi* (aq) + Mn04 (aq) Analysis: Oxidation-Half reation: Balancing atoms & charges: Mn*2(aq) Mn04 (aq) H20 - + H* + e Reduction-Half reation: Balancing atoms and charges: BiO3 (aq) H* + Bi* (aq) e H20 Balancing electrons lost & gained Multiply oxidation-half reaction by e's Multiply reduction-half reaction by es Final balanced equation: Continue nextarrow_forward3. What does the sum of oxidation numbers need to equal for a charged compound? The charge on the compound Zero The largest oxidation number The smallest oxidation number GET IT NOW New version available! (3.0.220)arrow_forward
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