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(B) The energy of an electron in the $n^{th}$ orbit is given by $E_{n} = -R_{H} 	imes \frac{Z^{2}}{n^{2}}$. The energy difference between the first $

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$9.835 	imes 10^{5}$

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(B) The energy of an electron in the $n^{th}$ orbit is given by $E_{n} = -R_{H} 	imes \frac{Z^{2}}{n^{2}}$. The energy difference between the first $(n=1)$ and second $(n=2)$ orbit for a hydrogen atom $(Z=1)$ is $\Delta E = E_{2} - E_{1} = R_{H} 	imes \left[ \frac{1}{1^{2}} - \frac{1}{2^{2}} ight]$. Given $R_{H} = 2.18 	imes 10^{-11} \ ergs = 2.18 	imes 10^{-18} \ J$. $\Delta E = 2.18 	imes 10^{-18} 	imes \left[ 1 - \frac{1}{4} ight] = 2.18 	imes 10^{-18} 	imes 0.75 = 1.635 	imes 10^{-18} \ J \ atom^{-1}$. To convert to $J \ mol^{-1}$, multiply by Avogadro's number $(N_{A} = 6.022 	imes 10^{23} \ mol^{-1})$: $\Delta E = 1.635 	imes 10^{-18} 	imes 6.022 	imes 10^{23} \approx 9.846 	imes 10^{5} \ J \ mol^{-1}$. Rounding to the provided option, the correct answer is $9.835 	imes 10^{5} \ J \ mol^{-1}$.

The energy required by electrons, present in the first Bohr orbit of hydrogen atom to be excited to the second Bohr orbit is . . . . . . $J \ mol^{-1}$.
Given: $R_{H} = 2.18 \times 10^{-11} \ ergs$

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The energy required by electrons, present in the first Bohr orbit of hydrogen atom to be excited to the second Bohr orbit is . . . . . . $J \ mol^{-1}$. Given: $R_{H} = 2.18 \times 10^{-11} \ ergs$