Advertisements
Advertisements
Question
Assertion: Cu is less reactive than hydrogen.
Reason: `E_((Cu^(2+))/(Cu))^Θ` is negative.
Options
Both assertion and reason are true and the reason is the correct explanation of assertion.
Both assertion and reason are true and the reason is not the correct explanation of assertion.
Assertion is true but the reason is false.
Both assertion and reason are false.
Assertion is false but reason is true.
Solution
Assertion is true but the reason is false.
Explanation:
Cu is less reactive than hydrogen because E°u2+ Cu is positive.
APPEARS IN
RELATED QUESTIONS
Can copper sulphate solution be stored in an iron vessel? Explain.
Calculate emf of the following cell at 25 °C :
Fe|Fe2+(0.001 M)| |H+(0.01 M)|H2(g) (1 bar)|Pt (s)
E°(Fe2+| Fe)= −0.44 V E°(H+ | H2) = 0.00 V
Depict the galvanic cell in which the reaction \[\ce{Zn(s) + 2Ag+(aq) → Zn^{2+}(aq) + 2Ag(s)}\] takes place. Further show:
- Which of the electrode is negatively charged?
- The carriers of the current in the cell.
- Individual reaction at each electrode.
Galvanic or a voltaic cell converts the chemical energy liberated during a redox reaction to ____________.
Standard hydrogen electrode operated under standard conditions of 1 atm H2 pressure, 298 K, and pH = 0 has a cell potential of ____________.
Which cell will measure standard electrode potential of copper electrode?
Use the data given in below find out which of the following is the strongest oxidising agent.
`"E"_("Cr"_2"O"_7^(2-)//"Cr"^(3+))^⊖`= 1.33 V `"E"_("Cl"_2//"Cl"^-)^⊖` = 1.36 V
`"E"_("MnO"_4^-//"Mn"^(2+))^⊖` = 1.51 V `"E"_("Cr"^(3+)//"Cr")^⊖` = - 0.74 V
The positive value of the standard electrode potential of Cu2+/Cu indicates that:
(i) this redox couple is a stronger reducing agent than the H+/H2 couple.
(ii) this redox couple is a stronger oxidising agent than H+/H2 .
(iii) Cu can displace H2 from acid.
(iv) Cu cannot displace H2 from acid.
What does the negative sign in the expression `"E"^Θ ("Zn"^(2+))//("Zn")` = − 0.76 V mean?
Represent the cell in which the following reaction takes place.The value of E˚ for the cell is 1.260 V. What is the value of Ecell?
\[\ce{2Al (s) + 3Cd^{2+} (0.1M) -> 3Cd (s) + 2Al^{3+} (0.01M)}\]