The nitrogen-to-hydrogen single bond energy is 389 kJ/mol in NH3. What is the minimum frequency of radiation having the necessary energy to break this bond?
I would convert 389 kJ/mol to J, then to molecules. That would be 389 kJ/mol x (1000 J/kJ) x (1 mole/6.022E23 molecule) = ?? J/molecule. Then
E = h*frequency.
To determine the minimum frequency of radiation required to break the nitrogen-to-hydrogen single bond in NH3, we can use the equation:
E = hf
where:
E = energy required to break the bond (in joules)
h = Planck's constant (6.626 x 10^-34 J∙s)
f = frequency of the radiation (in Hz)
First, let's convert the bond energy from kJ/mol to J/molecule:
Bond energy = 389 kJ/mol = 389,000 J/mol
Next, we need to convert the bond energy per mole to energy per molecule. Since there is one mole of NH3 in the bond, we can divide the bond energy by Avogadro's number (6.022 x 10^23 mol^-1):
Energy per molecule = 389,000 J/mol ÷ (6.022 x 10^23 mol^-1) ≈ 6.46 x 10^-19 J/molecule
Now we can calculate the minimum frequency using the equation. Rearranging the equation, we have:
f = E / h
Substituting the values:
f = 6.46 x 10^-19 J/molecule ÷ (6.626 x 10^-34 J∙s)
Calculating the frequency:
f ≈ 9.76 x 10^14 Hz
Therefore, the minimum frequency of radiation needed to break the nitrogen-to-hydrogen single bond in NH3 is approximately 9.76 x 10^14 Hz.
To determine the minimum frequency of radiation required to break the nitrogen-to-hydrogen single bond in NH3, we need to use the equation E = hν, where E is the energy, h is Planck's constant, and ν is the frequency of radiation.
First, we need to convert the bond energy from kJ/mol to joules per bond. Since one mole contains Avogadro's number (6.022 × 10^23) of bonds, we divide the bond energy by Avogadro's number. Thus, the bond energy per bond is:
E = 389 kJ/mol / (6.022 × 10^23) bonds/mol ≈ 6.46 × 10^-19 J/bond
Next, we can use this energy value to calculate the minimum frequency of radiation required to break the bond. Rearranging the equation E = hν, we have:
ν = E / h
Plugging in the values, we get:
ν = (6.46 × 10^-19 J/bond) / (6.626 × 10^-34 J·s) ≈ 9.75 × 10^14 Hz
Therefore, the minimum frequency of the radiation needed to break the nitrogen-to-hydrogen single bond in NH3 is approximately 9.75 × 10^14 Hz.