One requires `11eV` of energy to dissociate a carbon monoxide molecule into carbon and oxygen atoms. The minimum frequency of the appropriate electromagnetic radiation to achieve the dissociation lies in.

Options

A. visible region
B. infrared region
C. ultraviolet region
D. microwave region

Explanation

To find the minimum frequency of electromagnetic radiation required to dissociate a carbon monoxide molecule into carbon and oxygen atoms, we can follow these steps:

### Step-by-Step Solution:

1. **Identify the Energy Required for Dissociation**:
The energy required to dissociate a carbon monoxide (CO) molecule is given as \( E = 11 \, \text{eV} \).

2. **Convert Electron Volts to Joules**:
To convert the energy from electron volts to joules, we use the conversion factor:
\[ 1 \, \text{eV} = 1.6 \times 10^{-19} \, \text{J} \]
Therefore, the energy in joules is:
\[ E = 11 \, \text{eV} \times 1.6 \times 10^{-19} \, \text{J/eV} = 1.76 \times 10^{-18} \, \text{J} \]

3. **Use the Energy-Frequency Relation**:
The relationship between energy (E), frequency (ν), and Planck's constant (h) is given by:
\[ E = h \nu \]
Rearranging this formula to find frequency gives:
\[ \nu = \frac{E}{h} \]

4. **Substitute the Values**:
The value of Planck's constant \( h \) is approximately \( 6.63 \times 10^{-34} \, \text{J s} \). Now substituting the values we have:
\[ \nu = \frac{1.76 \times 10^{-18} \, \text{J}}{6.63 \times 10^{-34} \, \text{J s}} \approx 2.65 \times 10^{15} \, \text{Hz} \]

5. **Determine the Range of Electromagnetic Radiation**:
The frequency \( 2.65 \times 10^{15} \, \text{Hz} \) falls within the range of ultraviolet (UV) radiation, which is approximately \( 10^{14} \, \text{Hz} \) to \( 10^{17} \, \text{Hz} \).

### Conclusion:
The minimum frequency of the appropriate electromagnetic radiation required to dissociate a carbon monoxide molecule is approximately \( 2.65 \times 10^{15} \, \text{Hz} \), which lies in the ultraviolet range.