NO2(g)+SO2(g)-->NO(g)+SO3(g) here NO2 act as a oxidising agent
In this reaction, potassium permanganate (KMnO4) acts as the oxidizing agent. It oxidizes oxalic acid (H2C2O4) to carbon dioxide and sulfuric acid (H2SO4) helps to provide the acidic conditions needed for the reaction to occur.
No, citric acid is not a reducing agent. It acts as a weak acid and does not typically participate in reduction-oxidation (redox) reactions as a reducing agent.
Sulfur dioxide (SO2) acts as a reducing agent because it can easily be oxidized to sulfuric acid (H2SO4) by gaining oxygen atoms. In this process, another substance is reduced by gaining electrons from SO2, making it a reducing agent.
Zinc is a transition element with general oxidation state as +2. It gets easily oxidised to its oxidation state of +2 by elements which are less reactive than zinc . For example: 2Zn + H2O --> Zn2O + H2
No, iodine is not an oxidizing agent. It typically acts as a reducing agent, meaning it tends to gain electrons rather than lose them in chemical reactions.
In this reaction, potassium permanganate (KMnO4) acts as the oxidizing agent. It oxidizes oxalic acid (H2C2O4) to carbon dioxide and sulfuric acid (H2SO4) helps to provide the acidic conditions needed for the reaction to occur.
2H2S(g) + SO2(g) --> 2H2O + 3S Fe2O3 catalyst and temperature 673K
Yes, MnO2 is an oxidizing agent as it can accept electrons from other substances, causing them to be oxidized in a chemical reaction. It commonly acts as a strong oxidizing agent in various chemical reactions.
No, citric acid is not a reducing agent. It acts as a weak acid and does not typically participate in reduction-oxidation (redox) reactions as a reducing agent.
S+O2->SO2 Oxidation no. of sulphur changes from 0 to +4. Due to presence of d-orbitals(vacant) sulphur can extend its covalency & show oxidation states till +6, which is stable in sulphur (eg: SF6). Hence it acts as a reducing agent. Te+O2->TeO2 Oxidation no. of Te changes from 0 to +4. Unlike sulphur Te cannot show +6 oxidation state as it is highly unstable due to inert pair effect. Therefore there can only be a decrease in it oxidation state (it can decrease to -2, +2). Hence it acts as an oxidising agent.
Vitamin C acts as an antioxidant by reducing the concentration of oxygen. This is possible as it is a reducing agent.
Sulfur dioxide (SO2) acts as a reducing agent because it can easily be oxidized to sulfuric acid (H2SO4) by gaining oxygen atoms. In this process, another substance is reduced by gaining electrons from SO2, making it a reducing agent.
Zinc is a transition element with general oxidation state as +2. It gets easily oxidised to its oxidation state of +2 by elements which are less reactive than zinc . For example: 2Zn + H2O --> Zn2O + H2
No, iodine is not an oxidizing agent. It typically acts as a reducing agent, meaning it tends to gain electrons rather than lose them in chemical reactions.
In a redox titration using potassium permanganate, the permanganate ion (MnO4-) acts as the oxidizing agent while the other substance being titrated acts as the reducing agent. The endpoint is reached when all the reducing agent has been consumed, leading to a color change from purple to colorless or light pink. The volume of potassium permanganate solution required to reach the endpoint is used to calculate the concentration of the reducing agent.
In the reaction Ca + Br2 → CaBr2, calcium acts as the reducing agent because it undergoes oxidation by losing electrons to bromine. This results in the formation of calcium bromide (CaBr2).
Yes, in combustion, oxygen acts as the oxidizing agent because it gains electrons from the fuel being burned. In corrosion, however, oxygen acts as the oxidizing agent as it accepts electrons from the metal, causing it to corrode or rust.