The energy difference between the ground state of an atom and its excited state is 3 × 10-19 J. What is the wavelength of the photon required for this transition?

Question

The energy difference between the ground state of an atom and its excited state is 3 × 10-19 J. What is the wavelength of the photon required for this transition? (A) 6.6 × 10-34 m (B) 3 × 10-8 m (C) 1.8 × 10-7 m (D) 6.6 × 10-7 m

Tardigrade Admin · Accepted Answer

Δ E=(hc/λ) λ=(6.6 × 10-34 J s × 3 × 108 m s-1/3 × 10-19 J) =6.6×10-7 m

Q. The energy difference between the ground state of an atom and its excited state is $3 \times 1 0^{- 19} J$ . What is the wavelength of the photon required for this transition?

$6.6 \times 1 0^{- 34} m$

$3 \times 1 0^{- 8} m$

$1.8 \times 1 0^{- 7} m$

$6.6 \times 1 0^{- 7} m$

$Δ E = \frac{h c}{λ}$
$λ = \frac{6.6 \times 1 0 ^{- 34} J s \times 3 \times 1 0 ^{8} m s ^{- 1}}{3 \times 1 0 ^{- 19} J}$
$= 6.6 \times 1 0^{- 7} m$

Q. The energy difference between the ground state of an atom and its excited state is 3×10−19J. What is the wavelength of the photon required for this transition?

6.6×10−34m

3×10−8m

1.8×10−7m

6.6×10−7m