Answer:
ν = 5,765x10¹⁴ Hz
λ = 520 nm
230,0 kJ/mole
Explanation:
To convert energy yo frequency you need to use:
E = hν
Where E is energy (3,820x10⁻¹⁹ J)
h is Planck's constant (6,626x10⁻³⁴ Js)
And ν is frequency, replacing ν = 5,765x10¹⁴ s⁻¹ ≡ 5,765x10¹⁴ Hz
To convert frequency to wavelength:
c = λν
Where s is speed of light (2,998x10⁸ ms⁻¹)
ν is frequency (5,765x10¹⁴ s⁻¹)
And λ is wavelength, replacing: λ = 5,200x10⁻⁷ ≡ 520 nm
If 1 photon produce 3,820x10⁻¹⁹ J, in mole of photons produce:
3,820x10⁻¹⁹ J ×
= 230040 J/mole ≡ 230,0 kJ/mole
I hope it helps!
The mass of the object can also be determined if the density and volume of an object are known.
the answer to your question is A
Answer:
icicle becausit sounds right
Explanation:
icicles because it sounds right
Answer:
Explanation:
We are asked to find the mass of a sample of metal. We are given temperatures, specific heat, and joules of heat, so we will use the following formula.
The heat added is 4500.0 Joules. The mass of the sample is unknown. The specific heat is 0.4494 Joules per gram degree Celsius. The difference in temperature is found by subtracting the initial temperature from the final temperature.
- ΔT= final temperature - initial temperature
The sample was heated <em>from </em> 58.8 degrees Celsius to 88.9 degrees Celsius.
- ΔT= 88.9 °C - 58.8 °C = 30.1 °C
Now we know three variables:
- Q= 4500.0 J
- c= 0.4494 J/g°C
- ΔT = 30.1 °C
Substitute these values into the formula.
Multiply on the right side of the equation. The units of degrees Celsius cancel.
We are solving for the mass, so we must isolate the variable m. It is being multiplied by 13.52694 Joules per gram. The inverse operation of multiplication is division, so we divide both sides by 13.52694 J/g
The units of Joules cancel.
The original measurements have 5,4, and 3 significant figures. Our answer must have the least number or 3. For the number we found, that is the ones place. The 6 in the tenth place tells us to round the 2 up to a 3.
The mass of the sample of metal is approximately <u>333 grams.</u>
