A student used a spectroscope to view the emission spectrum of Hg vapor, and plo

Question

A student used a spectroscope to view the emission spectrum of Hg vapor, and plotted her measured wavelengths (y - axis) vs, the actual wavelengths (x - axis). The actual wavelength of the most prominent line in the mission spectrum of Na is 589 nm. If the spectroscope used to prepare the calibration curve is used to view the emission spectrum of Na, what wavelength would be measured for this line ? Use the Rydberg equation to calculate delete E(in joules). Frequency (in S - 1) and wavelength (in nm) for the following Balmer series transition in hydrogen delta E (in joules for n outer = 4 and n inner = 2. Frequency (in S - 1) for n outer = 3 and n inner = 2. First, use the Rydberg equation to calculate delta E; use the absolute value of delta E in equation (1) to solve for the frequency. The wavelength (in nm) for n out = 5 and n inner = 2. After calculating delta E, take the absolute value, and solve for frequency using Equation (1). Use this frequency in Equation (2) to solve for the wavelength.

Explanation / Answer

E=hcR(1/n1^2 -1/n2^2) , n1=2, n2=4 E = 6.625 x10^-34 x 3 x 10^10 x 109677(1/2^2 -1/4^2) =2.18 x10^-18 Joules E=hv , v is frequency and v=E/h = 2.18 x10^-18 / 6.625 x10^-34 =3.29 x10^15 Hz v=3.29 x10^15 Hz wavelength = c/v = 3 x10^8/3.29 x10^15 Hz = 9.12 x10^ -8 m

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