Home
Class 12
CHEMISTRY
Assertion:Cu^(2+) ions get reduced more...

Assertion:`Cu^(2+)` ions get reduced more easily than `H^+` ions.
Reason: Standard electrode potential of copper is 0.34 V.

A

If both assertion and reason are true and reason is the correct explanation of assertion .

B

If both assertion and reason are true but reason is not the correct explanation of assertion .

C

If assertion is true but reason is false .

D

If both assertion and reason are false .

Text Solution

AI Generated Solution

The correct Answer is:
To solve the question, we need to analyze the assertion and reason provided: **Assertion:** `Cu^(2+)` ions get reduced more easily than `H^+` ions. **Reason:** The standard electrode potential of copper is 0.34 V. ### Step-by-Step Solution: **Step 1: Understand the Standard Electrode Potential** - The standard electrode potential (E°) is a measure of the tendency of a chemical species to be reduced. The higher the E° value, the greater the tendency for the species to gain electrons (be reduced). **Hint for Step 1:** Remember that a higher standard electrode potential indicates a stronger oxidizing agent. **Step 2: Identify the Standard Reduction Potentials** - The standard reduction potential for the reduction of `Cu^(2+)` to `Cu` is +0.34 V. - The standard reduction potential for the reduction of `H^+` to `H2` is 0 V. **Hint for Step 2:** Look up standard reduction potentials in a table to compare values. **Step 3: Compare the Standard Potentials** - Since +0.34 V (for `Cu^(2+)`) is greater than 0 V (for `H^+`), this indicates that `Cu^(2+)` is more likely to be reduced than `H^+`. **Hint for Step 3:** Compare the numerical values directly to determine which species is more easily reduced. **Step 4: Analyze the Assertion and Reason** - The assertion states that `Cu^(2+)` ions get reduced more easily than `H^+` ions, which is supported by the comparison of their standard potentials. - The reason provided states that the standard electrode potential of copper is 0.34 V, which is true and helps explain why the assertion is correct. **Hint for Step 4:** Ensure that both the assertion and reason are logically connected. **Step 5: Conclusion** - Since both the assertion and the reason are true, and the reason correctly explains the assertion, we conclude that the correct answer is option A: both assertion and reason are true, and the reason is the correct explanation of the assertion. **Final Answer:** Option A is correct.
Promotional Banner

Topper's Solved these Questions

  • ELECTROCHEMISTRY

    NCERT FINGERTIPS ENGLISH|Exercise Electrochemical Cell|1 Videos

  • ELECTROCHEMISTRY

    NCERT FINGERTIPS ENGLISH|Exercise Galvanic Cell|19 Videos

  • ELECTROCHEMISTRY

    NCERT FINGERTIPS ENGLISH|Exercise EXEMPLAR PROBLEMS|17 Videos

  • COORDINATION COMPOUNDS

    NCERT FINGERTIPS ENGLISH|Exercise Assertion And Reason|15 Videos

  • GENERAL PRINCIPLES AND PROCESSES OF ISOLATION OF ELEMENTS

    NCERT FINGERTIPS ENGLISH|Exercise Assertion And Reason|15 Videos

Similar Questions

Explore conceptually related problems

Assertion : Copper is unable to displace H_2 form dil. H_2 SO_4 Reason : The standard electrode potential for Cu^(2+)//Cu system is greater than that of H^+//1/2 H_2 system.

Assertion : Cu^(2+) ion is a coloured ion . Reason : Every ion with unpaired electron is coloured .

Assertion: Cu^(2+) is more stable than Cu^(+) Reason: Electrode potential is more important in determining stable oxidation state than electronic configuration.

The positive value of the standard electrode potential of Cu^(2+)//Cu indicates that.......

The potential associated. with each electrode is known as electrode potential. If the concentration of each species taking part in the electrode reaction is unity (if any gås appears in the electrode reaction, it is confined to 1 atmospheric pressure) and further the reaction is carried out at 298 K, then the potential of each electrode is said to be the standard electrode potential. By convention, the standard electrode potential of hydrogen electrode is 0:0 volt. The electrode potential value for each electrode process is a measure, of relative tendency of the active species in the process to remain in the oxidized / reduced form. A negative E^@ means that the redox couple is a stronger reducing agent than the H^(+)//H_2 couple. A positive E mears that the redox couple is a weaker reducing agent than. the H^(+)//H couple. The metal with greater positive value of standard reduction potentlal forms the oxide of greater thermal stability: Given the standard reduction potentials. E_(K^(+)//K)^(@)=-2.93V, E_(Ag^(+)//Ag)^(@)=+0.80V, E_(Hg^(+)//Hg)^(@)=0.79V E_(Mg^(+)//Mg)^(@)=-2.37V, E_(Cr^(3+)//Cr)^(@)=-0.74V The correct increasing order of reducing power is:

Assertion (A) : Galvanized iron does not rust. Reason (R): Zn has a more negative electrode potential than Fe .

The more positive the value of E^(θ) , the greater is the trendency of the species to get reduced. Using the standard electrode potential of redox coples given below find out which of the following is the strongest oxidising agent. E^(θ) values: Fe^(3+)//Fe^(2+) = +0.77 I_(2)(s)//I^(-) = +0.54 , Cu^(2+)//Cu = +0.34, Ag^(+)//A = 0.80V

The more positive the value of E^(θ) , the greater is the trendency of the species to get reduced. Using the standard electrode potential of redox coples given below find out which of the following is the strongest oxidising agent. E^(θ) values: Fe^(3+)//Fe^(2+) = +0.77 I_(2)(s)//I^(-) = +0.54 , Cu^(2+)//Cu = +0.34, Ag^(+)//Ag = 0.80V

The potential associated. with each electrode is known as electrode potential. If the concentration of each species taking part in the electrode reaction is unity (if any gås appears in the electrode reaction, it is confined to 1 atmospheric pressure) and further the reaction is carried out at 298 K, then the potential of each electrode is said to be the standard electrode potential. By convention, the standard electrode potential of hydrogen electrode is 0:0 volt. The electrode potential value for each electrode process is a measure, of relative tendency of the active species in the process to remain in the oxidized / reduced form. A negative E^@ means that the redox couple is a stronger reducing agent than the H^(+)//H_2 couple. A positive E mears that the redox couple is a weaker reducing agent than. the H^(+)//H couple. The metal with greater positive value of standard reduction potentlal forms the oxide of greater thermal stability: Which of the following oxides will be themally most stable?

The potential associated. with each electrode is known as electrode potential. If the concentration of each species taking part in the electrode reaction is unity (if any gås appears in the electrode reaction, it is confined to 1 atmospheric pressure) and further the reaction is carried out at 298 K, then the potential of each electrode is said to be the standard electrode potential. By convention, the standard electrode potential of hydrogen electrode is 0:0 volt. The electrode potential value for each electrode process is a measure, of relative tendency of the active species in the process to remain in the oxidized / reduced form. A negative E^@ means that the redox couple is a stronger reducing agent than the H^(+)//H_2 couple. A positive E mears that the redox couple is a weaker reducing agent than. the H^(+)//H couple. The metal with greater positive value of standard reduction potentlal forms the oxide of greater thermal stability: Which of the following metals will not displace hydrogen from water?