An energy value of \(3.313 \times 10^{-19}\) joules is needed to break a chemical bond. What is the wavelength of energy needed to break the bond?
(The speed of light, \(c\), is \(3.00 \times 10^{10}\) cm/sec; Planck’s constant, \(h\), is \(6.626 \times 10^{-34}\) J⋅sec).
A. \(5.00 \times 10^{18}\) cm
B. \(1.00 \times 10^{15}\) cm
C. \(2.00 \times 10^{5}\) cm
D. \(6.00 \times 10^{-5}\) cm
E. \(1.20 \times 10^{-8}\) cm
Can someone explain to me how to solve this step by step?
Answer (2)
You need two formulas. You need E = hf and v = wavelength x frequency. Plug in the values for the first formula. f = 3.3 x 10^-19/6.63 x 10^-34 and you get f = 0.5 x 10^15. Now plug in this number to the second equation. Wavelength = 3.00 x 10^10 cm/sex/0.5 x 10^15 and you get D) 6.00 x 10^-5 cm.
To determine the wavelength needed to break a chemical bond with an energy of 3.313 × 1 0 − 19 joules, we calculated the frequency using E = h f and then found the wavelength using c = f λ . The wavelength calculated is approximately 6.00 × 1 0 − 5 cm. Thus, the correct answer is D. 6.00 × 1 0 − 5 cm.
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