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 ragion

Explanation

To solve the problem of finding 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 problem states that the energy required to dissociate a carbon monoxide molecule is \( E = 11 \, \text{eV} \).

2. **Convert Electron Volts to Joules**:
We need to convert the energy from electron volts to joules since Planck's constant is in joules. The conversion factor is:
\[ 1 \, \text{eV} = 1.6 \times 10^{-19} \, \text{J} \]
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 Planck's Equation**:
The relationship between energy and frequency is given by Planck's equation:
\[ E = h \nu \]
where \( h \) is Planck's constant, approximately \( 6.626 \times 10^{-34} \, \text{J s} \) and \( \nu \) is the frequency.

4. **Rearrange for Frequency**:
Rearranging the equation to solve for frequency \( \nu \):
\[ \nu = \frac{E}{h} \]

5. **Substitute the Values**:
Substitute the values of \( E \) and \( h \) into the equation:
\[ \nu = \frac{1.76 \times 10^{-18} \, \text{J}}{6.626 \times 10^{-34} \, \text{J s}} \]

6. **Calculate the Frequency**:
Performing the calculation:
\[ \nu \approx 2.65 \times 10^{15} \, \text{Hz} \]

7. **Determine the Region of the Electromagnetic Spectrum**:
Frequencies of the order \( 10^{15} \, \text{Hz} \) correspond to the ultraviolet region of the electromagnetic spectrum.

### Final Answer:
The minimum frequency of the appropriate electromagnetic radiation to achieve the dissociation lies in the ultraviolet region.