Limiting Ionic Molar Conductivities
The limiting ionic molar conductivities can be defined as the molar conductivities of ions when they are infinitely diluted in a solution. It is denoted by the symbol λ^0 and is measured in siemens per meter squared per mole (S m^2 mol^-1). In this case, the limiting ionic molar conductivities of K+ and Cl- are given as 73.5 and 76.5 S m^2 mol^-1 respectively.

Molar Conductivity of KCl
The molar conductivity of a solution can be calculated by the equation:
Λm = λ^0+ - λ^0-

Where Λm is the molar conductivity of the solution, λ^0+ is the limiting ionic molar conductivity of the cation, and λ^0- is the limiting ionic molar conductivity of the anion. In this case, the molar conductivity of the 0.1M KCl solution is given as 130.0 S m^2 mol^-1.

Calculating Kohlrausch's Constant
To calculate Kohlrausch's constant, we need to rearrange the equation for molar conductivity:

Λm = λ^0+ + λ^0-

Since the molar conductivity of a solution is the sum of the limiting ionic molar conductivities of the cation and anion, we can rewrite the equation as:

Λm = λ^0K+ + λ^0Cl-

Substituting the given values:

130.0 = 73.5 + 76.5

130.0 = 150.0

This equation is not possible, as the molar conductivity of a solution cannot be greater than the sum of the limiting ionic molar conductivities. Therefore, there must be an error in the given data or calculations.

Conclusion
In conclusion, the given data and calculations do not align with the principles of molar conductivity and Kohlrausch's constant. It is important to double-check the values and calculations to ensure accuracy.