All categories

2 years ago

When an excited electron spontaneously emits a photon, which energy transformation takes place

2 answers:

7 0

When an excited electron spontaneously emits a photon, the energy transformation from potential to kinetic energy takes place.

If an atom is in an excited state means full of energy, it goes from higher energy level to lower energy level. The electron releasing energy in the form of a photon, which is emitted in a random direction.

When the electron returns to a low energy state, it releases the potential energy in the form of kinetic energy so we can conclude that the energy transformation from potential to kinetic energy takes place.

Learn more about excited electron here: brainly.com/question/81112

Learn more: brainly.com/question/25976890

notka56 [123]2 years ago

4 0

Given what we know, we can confirm that when an excited electron spontaneously emits a photon, the energy released is electromagnetic energy.

<h3>What is a Photon and what energy does it release when being emitted?</h3>

A photon is a particle.
This means that it is one of the smallest forms of matter that we can study.
Photons form electromagnetic fields.
Therefore, when being emitted by an electron, photons release electromagnetic energy.

Therefore, we can confirm that when an excited electron spontaneously emits a photon, the energy released is electromagnetic energy due to the properties of the photon being emitted.

To learn more about photons visit:

brainly.com/question/24309591?referrer=searchResults

You might be interested in

1.How many mL of 0.523 M HBr are needed to dissolve 8.60 g of CaCO3?

prohojiy [21]

Answer:

The answer to your question is:

Explanation:

1.-

HBr = 0.523 M V = ?

CaCO3 = 8.6 g

2HBr(aq) + CaCO₃(s) ⇒ CaBr₂(aq) + H₂O(l) + CO₂(g)

MW CaCO₃ = 40 + 12 + 48 = 100 g

MW HBr = 80 + 1 = 81 g

Molarity = moles / volume

100 g of CaCO₃ ---------------- 1 mol

8.6 g ---------------- x

x = (8.6 x 1) / 100

x = 0.086 moles

2 moles of HBr ----------------- 1 mol of CaCO₃

x ----------------- 0.086 moles

x = (0.086 x 2) / 1 = 0.172 moles of HBr

Volume = moles / molarity

Volume = 0.172/ 0.523 = 0.323 l or 323 ml of HBr

2.-

V = ? ml NaOH 0.487 M

V = 101 ml of 0.628 M MnSO₄

MnSO₄(aq) + 2NaOH(aq) ⇒ Mn(OH)₂(s) + Na₂SO₄(aq)

MW MnSO₄ = 55 g

MW NaOH = NaOH = 40 g

Moles = Molarity x volume

Moles = (0.628) x (0.101)

Moles = 0.065 moles of MnSO₄

1 mol of MnSO₄ ------------------ 2 moles of NaOH

0.065 ----------------- x

x = (0.065x 2) / 1

x = 0.131 moles of NaOH

Volume = moles / molarity

Volume = 0.131 / 0.487

Volume = 0.268 l or 268 ml of NaOH

4 0

3 years ago

Where does the greenhouse effect occur?

attashe74 [19]

Answer:

the greenhouse effect occurs in the earths atmosphere

7 0

3 years ago

The compound known as butylated hydroxytoluene, abbreviated as BHT, contains carbon, hydrogen, and oxygen. A 1.376 g sample of B

Scilla [17]

Answer:

C15H24O

Explanation:

TO GET THE EMPIRICAL FORMULA, WE NEED TO KNOW THE MASSES AND CONSEQUENTLY THE NUMBER OF MOLES OF EACH OF THE INDIVIDUAL CONSTITUENT ELEMENTS.

FIRSTLY, WE CAN GET THE MASS OF THE CARBON FROM THAT OF THE CARBON IV OXIDE. WE NEED TO KNOW THE NUMBER OF MOLES OF CARBON IV OXIDE GIVEN OFF. THIS CAN BE CALCULATED BY DIVIVDING THE MASS BY THE MOLAR MASS OF CARBON IV OXIDE. THE MOLAR MASS OF CARBON IV OXIDE IS 44G/MOL

<h3>HENCE, THE NUMBER OF MOLES OF CARBON IV OXIDE IS 4.122/44 WHICH EQUALS 0.094. SINCE THERE IS ONLY ONE ATOM OF CARBON IN CO2 THEN THEY HAVE EQUAL NUMBER OF MOLES AND THUS THE NUMBER OF MOLES OF CARBON IS 0.094. WE CAN THEN PROCEED TO CALCULATE THE MASS OF CO2 PRESENT. THIS CAN BE CALCULATED BY MULTIPLYING THE NUMBER OF MOLES BY THE ATOMIC MASS UNIT. THE ATOMIC MASS UNIT OF CARBON IS 12. HENCE, THE MASS OF CO2 PRESENT IS 12 * 0.094 = 1.128g</h3><h3></h3><h3>WE CAN NOW GET THE MASS OF THE HYDROGEN BY MULTIPLYING THE NUMBER OF MOLES OF WATER BY 2 AND ALSO ITS ATOMIC MASS UNIT</h3><h3></h3><h3>TO GET THE NUMBER OF MOLES OF WATER, WE SIMPLY DIVIDE THE MASS BY THE MOLAR MASS. THE MOLAR MASS OF WATER IS 18g/mol. The NUMBER OF MOLES IS THUS 1.350/18 = 0.075</h3><h3></h3><h3>THE NUMBER OF MOLES OF HYDROGEN IS TWICE THAT OF WATER SINCE IT CONTAINS 2 ATOMS PER MOLECULE OF WATER. ITS NUMBER OF MOLES IS THUS 0.075*2 = 0.15 MOLE</h3><h3></h3><h3>THE MASS OF HYDROGEN IS THUS 0.075 * 2 * 1 = 0.15g</h3><h3></h3><h3>WE CAN NOW FIND THE MASS OF OXYGEN BY SUBTRACTING THE MASSES OF HYDROGEN AND CARBON FROM THE TOTAL MASS.</h3><h3 /><h3>MASS OF OXYGEN = 1.376-0.15-1.128 = 0.098g</h3><h3 /><h3>THE NUMBER OF MOLES OF OXYGEN IS THUS 0.098/16 = 0.006125</h3><h3 /><h3>WE CAN NOW USE THE NUMBER OF MOLES TO OBTAIN THE EMPIRICAL FORMULA.</h3><h3 /><h3>WE DO THIS BY DIVIDING EACH BY THE SMALLEST NUMBER OF MOLES WHICH IS THAT OF THE OXYGEN.</h3><h3 /><h3>C = 0.094/0.006125 = 15</h3><h3>H = 0.15/0.006125 = 24</h3><h3>O = 1</h3><h3 /><h3>THE EMPIRICAL FORMULA IS THUS C15H24O</h3>

7 0

3 years ago

A sample of ch4o with a mass of 32.0 g contains __________ molecules of ch4o. group of answer choices 5.32 ´ 10-23 1.00 1.88 ´ 1

LekaFEV [45]

The correct option is (C) 6.02 X 10²³

A sample of CH₄O with a mass of 32.0 g contains <u>6.02 X 10²³</u> molecules of CH₄O.

To calculate the number of moles;

Molar mass of CH₄O = C + 4(H) + O

= 12.01 + 4(1.008) + 16

= 32.04 g/mol

So, 1 mol of CH₄O = 32.04 g of CH₄O

Given, 32.0 g of CH₄O

According to Avagadro's constant 1 mole of a substance contains 6.022× 10^23 particles (molecules, atoms or ions).

= (32.0 g/1)(1 mol CH₄O/32.04 g CH₄O)(6.02x10²³/1 mol CH₄O)

= 6.02 X 10²³ molecules of CH₄O

Hence, a sample of will contain number of molecules 6.02 X 10²³ molecules.

Learn more about the Moles calculation with the help of the given link:

brainly.com/question/21085277

#SPJ4

3 0

2 years ago

Which is the smallest atom in group 15?

VashaNatasha [74]

Answer:

Explanation:

Property Nitrogen Bismuth

Atomic radius (pm) 56 143

First Ionization energy (kJ/mol) 1402 703

Common Oxidation state(s) -3 to +5 +3

Ionic radius (pm) 146(-3) 103(+3)

6 0

3 years ago

Read 2 more answers