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jekas [21]
3 years ago
15

Certain atoms emit photons of light with an energy of 3.820 ✕ 10−19 J. Calculate the frequency (in Hz) and wavelength (in nm) of

one of these photons.
frequency Hz

and

wavelength nm

What is the total energy (in kJ) in 1 mole of these photons?

kJ
Chemistry
1 answer:
charle [14.2K]3 years ago
4 0

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 ×\frac{6,022x10^{23}}{1 mole} = 230040 J/mole ≡ 230,0 kJ/mole

I hope it helps!

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Valproic acid, used to treat seizures and bipolar disorder, is composed of C, H, and O. A 0.165-g sample is combusted to produce
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Answer:

The empirical formula is = C_4H_8O

The formula of Valproic acid = C_8H_{16}O_2

Explanation:

Mass of water obtained = 0.166 g

Molar mass of water = 18 g/mol

Moles of H_2O = 0.166 g /18 g/mol = 0.00922 moles

2 moles of hydrogen atoms are present in 1 mole of water. So,

<u>Moles of H = 2 x 0.00922 = 0.01844 moles </u>

Molar mass of H atom = 1.008 g/mol

<u>Mass of H in molecule = 0.01844 x 1.008 = 0.018588 g </u>

Mass of carbon dioxide obtained = 0.403 g

Molar mass of carbon dioxide = 44.01 g/mol

Moles of CO_2 = 0.403 g  /44.01 g/mol = 0.009157 moles

1 mole of carbon atoms are present in 1 mole of carbon dioxide. So,

<u>Moles of C = 0.009157 moles </u>

Molar mass of C atom = 12.0107 g/mol

<u>Mass of C in molecule = 0.009157 x 12.0107 = 0.11 g </u>

<u>Given that the Valproic acid only contains hydrogen, oxygen and carbon. </u>So,

Mass of O in the sample = Total mass - Mass of C  - Mass of H

Mass of the sample = 0.165 g

<u>Mass of O in sample = 0.165 - 0.11 - 0.018588 = 0.036412 g  </u>

Molar mass of O = 15.999 g/mol

<u>Moles of O  = 0.036412  / 15.999  = 0.002276 moles</u>

<u></u>

<u>Taking the simplest ratio for H, O and C as: </u>

<u>0.01844 : 0.002276 : 0.009157</u>

<u> = 8 : 1 : 4</u>

The empirical formula is = C_4H_8O

Molecular formulas is the actual number of atoms of each element in the compound while empirical formulas is the simplest or reduced ratio of the elements in the compound.

Thus,  

Molecular mass = n × Empirical mass

Where, n is any positive number from 1, 2, 3...

Mass from the Empirical formula = 4×12 + 8×1 + 16= 72 g/mol

Molar mass = 144 g/mol

So,  

Molecular mass = n × Empirical mass

144 = n × 72

<u>⇒ n = 2</u>

The formula of Valproic acid = C_8H_{16}O_2

7 0
3 years ago
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