Calculate the energy emitted when electrons of `1.0 g`1 of hydrogen transition giving spectrum lines of the lowest in the visible regain of its atomic spectrum
`R_(H) = 1.1 xx 10^(7) m^(-1) , c= 3 xx 10^(8) m s^(-1)` and `h = 6.62 xx 10^(-34) J s`

Explanation

To calculate the energy emitted when electrons of 1.0 g of hydrogen transition to give spectrum lines of the lowest in the visible region of its atomic spectrum, we will follow these steps:

### Step 1: Identify the Transition
The lowest energy transition in the visible region for hydrogen occurs in the Balmer series, specifically from the third energy level (n=3) to the second energy level (n=2).

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

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