Answer:
4.5 x 10¹⁴ Hz
666.7 nm
1.8 x 10⁵ J
The color of the emitted light is red
Explanation:
E = energy of photons of light = 2.961 x 10⁻¹⁹ J
f = frequency of the photon
Energy of photons is given as
E = h f
2.961 x 10⁻¹⁹ = (6.63 x 10⁻³⁴) f
f = 4.5 x 10¹⁴ Hz
c = speed of light = 3 x 10⁸ m/s
λ = wavelength of photon
Using the equation
c = f λ
3 x 10⁸ = (4.5 x 10¹⁴) λ
λ = 0.6667 x 10⁻⁶ m
λ = 666.7 x 10⁻⁹ m
λ = 666.7 nm
n = number of photons in 1 mole = 6.023 x 10²³
U = energy of 1 mole of photons
Energy of 1 mole of photons is given as
U = n E
U = (6.023 x 10²³) (2.961 x 10⁻¹⁹)
U = 1.8 x 10⁵ J
The color of the emitted light is red
Answer:
a. A = 0.735 m
b. T = 0.73 s
c. ΔE = 120 J decrease
d. The missing energy has turned into interned energy in the completely inelastic collision
Explanation:
a.
4 kg * 10 m /s + 6 kg * 0 m/s = 10 kg* vmax
vmax = 4.0 m/s
¹/₂ * m * v²max = ¹/₂ * k * A²
m * v² = k * A² ⇒ 10 kg * 4 m/s = 100 N/m * A²
A = √1.6 m ² = 1.26 m
At = 2.0 m - 1.26 m = 0.735 m
b.
T = 2π * √m / k ⇒ T = 2π * √4.0 kg / 100 N/m = 1.26 s
T = 2π *√ 10 / 100 *s² = 1.99 s
T = 1.99 s -1.26 s = 0.73 s
c.
E = ¹/₂ * m * v²max =
E₁ = ¹/₂ * 4.0 kg * 10² m/s = 200 J
E₂ = ¹/₂ * 10 * 4² = 80 J
200 J - 80 J = 120 J decrease
d.
The missing energy has turned into interned energy in the completely inelastic collision
I think it's C, longer wave length.
Answer:
The most common oxidation numbers for a given element
There must be a equal opposite reaction.
E=mv2