Redox Reactions
Redox reactions, short for reduction-oxidation reactions, are fundamental chemical processes that play a pivotal role in various natural and industrial contexts. These reactions involve the transfer of electrons between reactants, where one substance undergoes oxidation (loses electrons) while another undergoes reduction (gains electrons). Redox reactions are ubiquitous in biological systems, powering cellular respiration and photosynthesis, as well as in industrial applications like batteries and corrosion processes. Understanding the principles of redox reactions is crucial for comprehending diverse fields, ranging from chemistry and biology to energy storage and environmental science.
Questions
- Balance the following redox reaction in acidic solution?
- Can you represent the oxidation of sulfite ion, #SO_3^(2-)#, to give sulfate ion, #SO_4^(2-)#, accompanied by the reduction of #Cu^(2+)# to copper metal?
- Permanganate ion is reduced to #MnO_2#, and ammonia is oxidized to nitrate ion. Can you write a balanced chemical equation to represent the redox process?
- What is the lead discharge battery?
- Redox refers to a substance gaining an electron and releasing what?
- How goes the redox reaction of burning methane?
- 2.0 g of molybdenum (Mo) combines with oxygen to form 3.0 g of a molybdenum oxide. What is the equivalent weight of Mo in this compound?
- How does charge conservation apply in redox reactions?
- How do you determine the oxidizing or reducing agent in a redox equation?
- If the redox reaction in an electrochemical cell occurs naturally and produces electrical energy, what type of cell is it?
- Aluminum, #"Al"#, produces #"H"_2# bubbles when immersed in #"HCl"#, mercury, #"Hg"# does not. Which is the strongest reducer?
- Are oxidation reactions always exothermic?
- In the redox reaction #AgNO_3 + Na -> NaNO_3 + Ag#, which element has been reduced?
- Iron is extracted from iron ore. Part of the process involves reduction of the ore with carbon monoxide. Iron ore contains iron oxide (#Fe_2O_3#). How would you write a balanced equation for the reaction of iron oxide with carbon monoxide?
- What does the oxidizing agent do in a redox reaction?
- How do you balance redox equations using the oxidation number change method?
- Is the reaction between natrium hydroxide and and hydrogen chloride a redox process?
- In terms of electron gain and loss, and half equations why is Cl2+2NaI -> 2NaCl+I2 a redox reaction? (6 mark question)
- How do we represent the reaction of hydrochloric acid with stoichiometric calcium carbonate? Do we need to consider oxidation states?
- Why is the oxidation of #Mn^(2+)# in ACIDIC media represented differently to the oxidation of #Mn^(2+)# in an ALKALINE medium? What do we mean by #H^+# or #H_3O^+#?