1. Use the Rydberg equation and your measured wavelengths to determine the energ

Question

1. Use the Rydberg equation and your measured wavelengths to determine the energy transitions associated with each of your observed wavelengths for hydrogen. In other words, calculate the excited state energy level (n2) for each of your observed wavelengths for hydrogen. n has integer values; so, calculate it first with appropriate significant digits, then round it to an integer.

2. Using your wavelengths and the n2 integer values determined in the previous question, calculate an experimental value of the Rydberg constant for each wavelength by solving the Rydberg equation for R. Average the values and determine the % error in this value compared to the literature value of the constant.

Wavelength values of Hydrogen:

423.50 nm, 480.20nm, and 650.0 nm

Explanation / Answer

1.Rydberg equation is : Energy= 1/wavelength =R(1/n2f1/n2i)

suppose ni= 1 for hydrogen as not mentioned.

1. So, at wavelength = 423.5nm = 423E-9m

1/423E-9m = 1.09E7m1 (1/n2f)

nf = 2.15 = 2

2 at wavelength = 480.2nm = 480.2E-9m

1/480.2E-9m = 1.09E7m1 (1/n2f)

nf = 2.3= 2

3 at wavelength = 650nm = 650E-9m

1/650E-9m = 1.09E7m1 (1/n2f)

nf = 2.67= 3

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