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V125BC [204]
2 years ago
14

In a chemical process, you need to force a compound to bond with a halogen, causing it to lose hydrogen. Which type of reaction

do you need to perform?
Chemistry
1 answer:
Kazeer [188]2 years ago
5 0
Answer is Halogenation because Halogenation is a type of substitution reaction in which a hydrogen atom is replaced by a halogen atom in a molecule.
The molecule looses its hydrogen atom as the halogen is introduced into the molecule. This sort of reaction is very common in organic chemistry. Many hydrocarbons can be halogenated in the presence of light.
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In a molecule, how do we show what types of atoms are there and how many atoms there are of each type. ​
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Chemical or molecular formulas? Symbols from the periodic table are used to show which atoms are present in a molecule and subscripts show the number of atoms and of each type in the molecule.
6 0
3 years ago
An atomic number stands for the number of _____. neutrons in the nucleus of an atom protons in the nucleus of an atom valence el
Effectus [21]

Answer:

atoms or electrons

Explanation:

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3 years ago
Hello summer roses~<br>help me with these questions ​
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Answer:

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3 0
2 years ago
How many neutrons are present in an atom of element C?
Stolb23 [73]

Answer:

six  neutrons

Explanation:

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4 0
2 years ago
Read 2 more answers
How much energy is required to raise the temperature of 3 kg of iron from 20° C to 25°C? Use the table below and this equation:
ElenaW [278]

The energy required to raise the temperature of 3 kg of iron from 20° C to 25°C is 6,750 J( Option B)

<u>Explanation:</u>

Given:

Specific Heat capacity of Iron= 0.450 J/ g °C

To Find:

Required Energy to raise the Temperature

Formula:

Amount of energy required is given by the formula,

Q = mC (ΔT)

Solution:

M = mass of the iron in g

So 3 kg = 3000 g

C = specific heat of iron = 0.450 J/ g °C [ from the given table]

ΔT = change in temperature = 25° C - 20°C = 5°C

Plugin the values, we will get,

Q = 3000 g ×  0.450 J/ g °C ×  5°C

 = 6,750 J

So the energy required is 6,750 J.

7 0
3 years ago
Read 2 more answers
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