$C_{11}H_{18}O_{12}$The value of the Rydberg constant ($R_H$) is $2.18 \times 10^{-18} \, \text{J}$. The velocity of an electron having mass $9.1 \times 10^{-31} \, \text{kg}$ in Bohr's first orbit of the hydrogen atom is:$\dots \times 10^5 \, \text{ms}^{-1}$ (nearest integer).

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Using the formula for the velocity of an electron: $ v = 2.18 \times 10^6 \times \frac{Z}{n} $ For hydrogen ($ Z = 1, n = 1 $): $ v = 2.18 \times 10^6 \times \frac{1}{1} = 2.18 \times 10^6 \, \text{ms}^{-1} \approx 22 \times 10^5 \, \text{ms}^{-1} $

\(C_{11}H_{18}O_{12}\)The value of the Rydberg constant (\(R_H\)) is \(2.18 \times 10^{-18} \, \text{J}\). The velocity of an electron having mass \(9.1 \times 10^{-31} \, \text{kg}\) in Bohr's first orbit of the hydrogen atom is:\(\dots \times 10^5 \, \text{ms}^{-1}\) (nearest integer).

Correct Answer: 22

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