E° for the reaction Fe+Zn2+ =Zn+Fe2+ is 0.35V. The given cell reaction is
Answers
Solution :
The balanced cell reaction will be,
Zn(s)+Fe^{2+}(aq)\rightarrow Zn^{2+}(aq)+Fe(s)
Here, zinc (Zn) undergoes oxidation by loss of electrons and thus act as anode. Iron (Fe) undergoes reduction by gain of electrons and thus act as cathode.
Now we have to calculate the EMF for the cell reaction.
As we are given the standard oxidation cell potential. Thus, the reduction cell potential will be,
E^o_{[Fe^{2+}/Fe]}=-0.44V
E^o_{[Zn^{2+}/Zn]}=-0.76V
E^o=E^o_{[Zn^{2+}/Zn]}-E^o_{[Fe^{2+}/Fe]}
E^o=(-0.76V)-(-0.44V)=-0.32V
Therefore, the EMF for the cell reaction will be, -0.32 V
Answer:
The square root of 2, or the (1/2)th power of 2, written in mathematics as √2 or 21⁄2, is the positive algebraic number that, when multiplied by itself, equals the number 2. Technically, it is called the principal square root of 2, to distinguish it from the negative number with the same property.
Geometrically the square root of 2 is the length of a diagonal across a square with sides of one unit of length; this follows the Pythagorean theorem. It was probably the first number known to be irrational.[citation needed]
As a good rational approximation for the square root of two, with a reasonably small denominator, the fraction 99/70 (≈ 1.4142857) is sometimes used.
The sequence A002193 in the OEIS consists of the digits in the decimal expansion of the square root of 2, here truncated to 65 decimal places: