Light shines through atomic hydrogen gas that was initially in its ground state. You observe that after awhile much of the hydrogen gas has been excited to its $n = 5$ state. What wavelength of light entering the gas caused this excitation? $\left( c = 3.00 \times 10 8 } \mathrm {~m} / \mathrm { s } , h = 6.626 \times 10 - 34 \mathrm {~J} \cdot \mathrm { s } , 1 \mathrm { eV } = 1.60 \times \right.$ 10-19 J)
A) $2280 \mathrm {~nm}$
B) $91.4 \mathrm {~nm}$
C) $95.2 \mathrm {~nm}$
D) $110 \mathrm {~nm}$

Question

Light shines through atomic hydrogen gas that was initially in its ground state. You observe that after awhile much of the hydrogen gas has been excited to its

n = 5

state. What wavelength of light entering the gas caused this excitation?

\left( c = 3.00 \times 10&lt;sup&gt; 8 &lt;/sup&gt;} \mathrm {~m} / \mathrm { s } , h = 6.626 \times 10&lt;sup&gt; - 34&lt;/sup&gt; \mathrm {~J} \cdot \mathrm { s } , 1 \mathrm { eV } = 1.60 \times \right.

10-19 J)
A)

2280 \mathrm {~nm}

B)

91.4 \mathrm {~nm}

C)

95.2 \mathrm {~nm}

D)

110 \mathrm {~nm}

Quizplus · Accepted Answer

The Answer of Light shines through atomic hydrogen gas that was initially in its ground state. You observe that after awhile much of the hydrogen gas has been excited to its $n = 5$ state. What wavelength of light entering the gas caused this excitation? $\left( c = 3.00 \times 10⁸} \mathrm {~m} / \mathrm { s } , h = 6.626 \times 10^{- 34} \mathrm {~J} \cdot \mathrm { s } , 1 \mathrm { eV } = 1.60 \times \right.$ 10^-19 J) A) $2280 \mathrm {~nm}$ B) $91.4 \mathrm {~nm}$ C) $95.2 \mathrm {~nm}$ D) $110 \mathrm {~nm}$

Light Shines Through Atomic Hydrogen Gas That Was Initially in Its