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- Assertion H2SO4 is a strong oxidizing agent Reason class 11 . . . - Vedantu
H 2 S O 4 is a strong oxidizer Since H 2 S O 4 is a strong acid, it reacts with a weak amphoteric base water in dilute concentrations to produce H 3 O + ions However, since the condensed solution is very watery, it continues to form H 2 O
- Is sulfuric acid an oxidizing agent or reducing agent? Why?
If it is reduced in a chemical reaction, it will gain electrons The species that loses the electrons has been oxidised, and therefore sulfuric acid can be an oxidising agent (but never a reducing agent as S has no oxidation state greater than +6) For example: H2SO4 + 2H+ + 2Br- → Br2 + SO2 + H2O
- Which of the following can not act as reducingagent? (1) H2SO4 . . . - Filo
H2SO4 (Sulfuric Acid): Concentrated H2SO4 can act as an oxidizing agent rather than a reducing agent, especially when it is concentrated Therefore, it is not a good reducing agent HClO3 (Chloric Acid): HClO3 is a strong oxidizing agent and does not act as a reducing agent
- Give a reason why concentrated and not dil H2SO4 – behave as an . . .
H2SO4 act as a great affinity for water and hydration of cone H2SO4 is an exothermic reaction On the other hand dil H2SO4 has no affinity for water and hence cannot act as a hydrating agent
- H2SO4 = H + SO4 Redox Reaction - ChemicalAid
H2SO4 = 2H + SO4 is a redox reaction where O is oxidized and H, S are reduced H 2 SO 4 are reducing agents (i e they lost electrons) and H 2 SO 4, H 2 SO 4 are oxidizing agents (i e they gained electrons)
- Which of the following acts both as oxidising as well as reducing . . .
In \ (SO_2\), sulphur has a +4 oxidation state In \ (H_2SO_4\), Sulphur exhibits its highest oxidation state of +6 On the other hand in \ (H_2S\), sulphur exists in its lowest -2 oxidation state Thus, we can surmise that \ (SO_2\) could act as both an oxidising agent as well as a reducing agent Nitrogen exhibits its highest oxidation
- Is h2so4 an reducing agent?? - Brainly. in
To act a a reducing agent one should lose electrons i e; the atom should go from lower positive oxidation state to higher positive oxidation state As sulphur is already in it's maximum possible oxidation state in H2SO4, further loss of electrons is not possible So it can't act as a reducing agent Find Physics textbook solutions?
- What are the oxidizing and reducing agents in this redox reaction?
In the redox reaction H2SO4 (aq) + 2HI (aq) --> SO2 (g) + I2 (s) + 2H2O (l), sulfur in H2SO4 is oxidized, indicating that H2SO4 acts as the reducing agent Conversely, HI is oxidized to I2, making it the oxidizing agent
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