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GenaCL600 [577]
3 years ago
14

The third ionization energy of bromine is the energy required for which of the following processes?

Chemistry
1 answer:
Rzqust [24]3 years ago
3 0

Answer:

<u><em /></u>

  • <u><em>Br²⁺ (g)  → Br³⁺ (g) + e⁻</em></u>

Explanation:

1) The <u>first ionization energy</u> is the energy required to release an electron from a gas neutral atom.

Hence, this is the energy required for this process:

  • Br (g)  → B⁺ (g) + e⁻

2) The <u>second ionization energy </u>is the energy required to release an electron from a gas ion with charge 1+.

Hence, this is the energy required for this process:

  • Br⁺ (g)  → B²⁺ (g) + e⁻

3) The<em><u> third ionization energy</u></em> is the energy required to release an electron from a gas ion with charge +2.

Hence, this is the energy required for this process:

<u />

  • <u><em>Br²⁺ (g)  → B³⁺ (g) + e⁻</em></u>
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Evaluate this statement: Substances are made of two or more types of elements.
wolverine [178]

A MOLECULE IS MADE OF TWO OR MORE ELEMENTS CHEMICALLY COMBINED IS KNOWN AS A COMPUND.

A MOLECULE IS MADE OF TWO ATOMS IS JUST AN ELEMENT.

A MOLECULE MADE OF TWO OR MORE ELEMENTS IS KNOWN AS A COMPUND.

6 0
3 years ago
A 3.8-mol sample of KClO3 was decomposed according to the equation. How many moles of O2 are formed assuming 100% yield?
kari74 [83]

Answer:

5.7 moles of O2

Explanation:

We'll begin by writing the balanced decomposition equation for the reaction. This is illustrated below:

2KClO3 —> 2KCl + 3O2

From the balanced equation above,

2 moles of KClO3 decomposed to produce 3 moles of O2.

Next, we shall determine the number of mole of O2 produced by the reaction of 3.8 moles of KClO3.

Since 100% yield of O2 is obtained, it means that both the actual yield and theoretical yield of O2 are the same. Thus, we can obtain the number of mole of O2 produced as follow:

From the balanced equation above,

2 moles of KClO3 decomposed to produce 3 moles of O2.

Therefore, 3.8 moles of KClO3 will decompose to produce = (3.8 × 3)/2 = 5.7 moles of O2.

Thus, 5.7 moles of O2 were obtained from the reaction.

3 0
2 years ago
In which picture(s) will you find a state of matter that has particles who have more energy than liquid water?
kari74 [83]

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5 0
3 years ago
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Consider the reaction of diboron trioxide with carbon and chlorine. B2O3 (s) + 3C (s) + 3Cl2 (g) 2BCl3 (g) + 3CO (g) Determine t
Sholpan [36]

Answer:

Limiting reactant = B2O3

Amount of BCl3 formed = 468 g

Explanation:

The given reaction is:

B2O3 (s) + 3C (s) + 3Cl2 (g) \rightarrow 2BCl3 (g) + 3CO (g)

In order to identify the limiting reagent calculate the moles of B2O3, C and Cl2. The reagent with the lowest moles is the limiting reactant

Moles(B2O3)=\frac{Mass(B2O3)}{Mol.wt(B2O3)}=\frac{139g}{69.6g/mol}=1.997moles

Moles(C)=\frac{Mass(C)}{At.wt(C)}=\frac{87.8g}{12g/mol}=7.317moles

Moles(Cl2)=\frac{Mass(Cl2)}{Mol.wt(Cl2)}=\frac{650g}{70.9g/mol}=9.168moles

Since the moles of B2O3 < C < Cl2, the limiting reactant is B2O3

Based on the reaction stoichiometry:

1 mole of B2O3 produces 2 moles of BCl3

Hence, the number of moles of BCl3 produced under the experimental conditions = 2*1.997=3.994 moles

Mass(BCl3)= Moles* Mol.wt = 3.994 moles*117.17g/mol = 468 g

8 0
2 years ago
Is stannous fluoride ionic or covalent
laila [671]
Stannous flutoide is ionic
8 0
3 years ago
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