An energy value of 3.313 * 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 = 3.00 * 10¹⁰ cm/sec; Planck's constant = 6.626 * 10^{-34} J ⋅sec).

A. 5.00 * 10¹⁸ cm

B. 1.00 * 10¹⁵ cm

C. 2.00 * 10⁵ cm

D. 6.00 * 10^{-5}cm

E. 1.20 * 10^{-8} cm

Can someone explain me how to make this one step by step?

Question

Chemistry

Jan Shepard

22 February, 12:32

An energy value of 3.313 * 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 = 3.00 * 10¹⁰ cm/sec; Planck's constant = 6.626 * 10^{-34} J ⋅sec).

A. 5.00 * 10¹⁸ cm

B. 1.00 * 10¹⁵ cm

C. 2.00 * 10⁵ cm

D. 6.00 * 10^{-5}cm

E. 1.20 * 10^{-8} cm

Can someone explain me how to make this one step by step?

+3

Answers (1)

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Adams · Answer 1

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.