The ionisation enthalpy of hydrogen atom is 1.312 x106 J mol-1. The energy required to excite the electron in the atom from n = 1 to n = 2 is :

ΔE=E2−E1=−1.312×1064+1.312×106=9.84×105J mol−1

The ionisation enthalpy of hydrogen atom is 1.312 x106 J mol-1. The energy required to excite the electron in the atom from n = 1 to n = 2 is :

ΔE=E2−E1=−1.312×1064+1.312×106=9.84×105J mol−1

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The ionisation enthalpy of hydrogen atom is 1.312 x10⁶ J mol^-1. The energy required to excite the electron in the atom from n = 1 to n = 2 is :

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9.84 x 10⁵ J mol^-1

9.51 x 10⁵ J mol^-1

6.56 x 10⁵ J mol^-1

7.56 x 10⁵ J mol^-1

answer is A.

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$\begin{array}{l} ΔE = E_{2} - E_{1} = - \frac{1 .312 \times 10^{6}}{4} + 1 .312 \times 10^{6} \\ = 9 .84 \times 10^{5} J {mol}^{- 1} \end{array}$

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The ionisation enthalpy of hydrogen atom is 1.312 x106 J mol-1. The energy required to excite the electron in the atom from n = 1 to n = 2 is :

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The ionisation enthalpy of hydrogen atom is 1.312 x10⁶ J mol^-1. The energy required to excite the electron in the atom from n = 1 to n = 2 is :