Calculate the longest wavelength of light that can break a H-O bond. The bond enthalpy of formation is 463 kj/mol
http://butane.chem.uiuc.edu/pshapley/GenChem2/A4/2.html
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To calculate the longest wavelength of light that can break a H-O bond, we need to first determine the energy required to break the bond. We can then convert this energy into wavelength using the relationship between energy and wavelength.
1. Convert the bond enthalpy of formation from kilojoules per mole (kJ/mol) to joules (J) per molecule:
463 kJ/mol × (1000 J/1 kJ) = 463,000 J/mol
2. Utilize Avogadro's number (6.022 × 10^23 molecules/mol) to convert from J/mol to J per molecule:
463,000 J/mol ÷ (6.022 × 10^23 molecules/mol) = 7.689 × 10^-19 J
3. Use the formula E = hc/λ, where E is energy, h is Planck's constant (6.626 × 10^-34 J⋅s), c is the speed of light (3.00 × 10^8 m/s), and λ is the wavelength in meters.
Rearranging the formula to solve for wavelength (λ), we get: λ = hc/E
λ = (6.626 × 10^-34 J⋅s × 3.00 × 10^8 m/s) / (7.689 × 10^-19 J)
λ = 2.711 × 10^-6 meters
4. Convert the wavelength from meters to nanometers (nm) by multiplying by 10^9:
2.711 × 10^-6 meters × (10^9 nm/1 meter) = 2,711 nm
Therefore, the longest wavelength of light that can break a H-O bond is approximately 2,711 nm.
To calculate the longest wavelength of light that can break a H-O (hydrogen-oxygen) bond, we need to determine the energy required to break the bond. Let's start by converting the bond enthalpy of formation from kilojoules per mole (kJ/mol) to joules (J) per molecule.
1 kJ = 1000 J
Bond enthalpy of formation = 463 kJ/mol = 463,000 J/mol
To calculate the energy required to break a single H-O bond, we divide the bond enthalpy of formation by Avogadro's number (6.022 x 10^23 molecules/mol). This gives us the energy required to break the bond in one molecule.
Energy required to break one H-O bond = 463,000 J/mol / (6.022 x 10^23 molecules/mol)
Now we can use the energy-wavelength relationship to find the longest wavelength of light that can break the bond. The energy of a photon can be calculated using the equation:
Energy (E) = Planck's constant (h) × speed of light (c) / wavelength (λ)
Rearranging the equation to solve for wavelength:
Wavelength (λ) = Planck's constant (h) × speed of light (c) / Energy (E)
Plugging in the value of energy required to break the bond, we can calculate the longest wavelength of light. The Planck's constant (h) is approximately 6.626 x 10^(-34) J·s, and the speed of light (c) is approximately 3.0 x 10^8 m/s.
Let's perform the calculation:
Wavelength (λ) = (6.626 x 10^(-34) J·s × 3.0 x 10^8 m/s) / Energy required to break one H-O bond
Please provide the value of the energy required to break one H-O bond, and I'll calculate the longest wavelength of light that can break the bond.