All categories

3 years ago

What is the approximate frequency of a photon having an energy 3.2 * 10^-24 J? (h = 6.610^-34 Js)

Chemistry

1 answer:

hichkok12 [17]3 years ago

4 0

The Planck’s Equation states that

E = hv

E stands for energy measured in Joules

v stands for frequency measured in s^-1 or Hertz (Hz)- 1Hz .

h is Planck’s constant which is equivalent to 6.626x10-34 J.s

The Planck's equation states that the energy of a photon, is directly proportional to its frequency (v), by a constant factor (h).

Given:

E=3.2 * 10^-24 J

h= 6.626x10-34 J.s

Now we know that

E=hv

Thus substituting the given values we get

v=3.2 * 10^-24 /6.626x10-34

v=48 x 10^9 s^-1

You might be interested in

How was the noble gas argon discovered

Mashcka [7]

Argon was discovered by Lord Rayleigh and Sir William Ramsay in 1894. It was isolated by examination of the residue obtained by removing nitrogen, oxygen, carbon dioxide, and water from clean air.

4 0

3 years ago

Read 2 more answers

Write the word and balanced chemical equations for the reaction between:

kupik [55]

Answer:

Alumminum hydroxide reacts with sulfuric acid as follows: 2Al(OH)3+H2SO4-->Al2(SO4)+6H2O.

Explanation:

plz mark as brainlist

7 0

3 years ago

Which kind of bond occurs when two atoms share an electron

Dmitriy789 [7]

Answer:

<h2>Covalent bond</h2>

Explanation:

6 0

4 years ago

2. A sample of table sugar (sucrose, C12H22O11) has a mass of 1.202 g.

Snezhnost [94]

Explanation:

Given mass of sugar = 1.202 g

Molar mass of the sugar , $C_{12}H_{22}O_{11}$ = 342.29 g/mol

a) Number of moles of sugar

$\text{number of moles}=\frac{\text{given mass of sugar}}{\text{molar mass of sugar}}=\frac{1.202 g}{342.29g/mol}=0.0035 mol$

Number of moles of sugar in 1.202 grams is 0.0035 moles

b)Moles of each element in $C_{12}H_{22}O_{11}$

In a molecular formula of sugar there are 12 carbon, 22 hydrogen and 11 oxygen atoms

Moles of an element in molecule =

number of atoms of that element in a molecular formula × number of moles of compound

Moles of carbon = 12 × 0.0035 = 0.042 moles

Similarly

Moles of hydrogen = 22 × 0.0035 = 0.077 moles

Moles of oxygen =11 × 0.0035 = 0.0385 moles

c) Number of atoms of each type in $C_{12}H_{22}O_{11}$

$\text{Number of atoms}=\text{number of moles of that atom in a molecular formula}\times \text{Avogadro number}$

Number of carbon atoms = $0.042 mole\times 6.022 \times 10^{23}=2.52\times 10^{22} atoms$

Number of hydrogen = $0.077mole\times 6.022 \times 10^{23}=4.63\times 10^{22} atoms$

Number of oxygen atoms = $0.0385 mole\times 6.022 \times 10^{23}=2.31\times 10^{22} atoms$

7 0

3 years ago

Read 2 more answers

What is the total number of orbitals found in the second energy level?

erik [133]

Principal Energy Light Type of sub level Maximum number of electrons
P 8
2
S 18
3
P
Hope It really Helps

6 0

3 years ago

What is the approximate frequency of a photon having an energy 3.2 * 10^-24 J? (h = 6.6*10^-34 J*s)

What is the approximate frequency of a photon having an energy 3.2 * 10^-24 J? (h = 6.610^-34 Js)