Calculate the energy emitted when electrons of 1.0 g atom of hydrogen undergo transition giving the spectral line of largest energy in the visible region of its atomic spectrum. `(R_H = 1.1 xx 10^7 m^(-1), c = 3 xx 10^8 m s^(-1), h = 6.62 xx 10^(-34) J s)`

Explanation

To calculate the energy emitted when electrons of 1.0 g atom of hydrogen undergo a transition giving the spectral line of largest energy in the visible region of its atomic spectrum, we can follow these steps:

### Step 1: Understand the Transition
The largest energy transition in the visible region for hydrogen occurs in the Balmer series, specifically from n=3 to n=2.

### Step 2: Use the Rydberg Formula
The Rydberg formula for the wavelength of the emitted light is given by:
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