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Lilit [14]
2 years ago
7

Substances that cause the oxidation of other substances are

Chemistry
1 answer:
svp [43]2 years ago
4 0
<h3>SUBSTANCE</h3>

==============================

\large  \sf\underline{Question:}

  • Substances that cause the oxidation of other substances are;

==============================

\large  \sf\underline{Answer:}

\qquad \qquad \huge \bold{Option \:  B}

==============================

\large  \sf\underline{Explanation:}

  • Substances that cause the oxidation of other substances are oxidizing agents.

==============================

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Nitrosyl fluoride has the chemical formula NOF. Nitrogen has five valence electrons, oxygen has six, and fluorine has seven. Com
alexira [117]

Answer:

Watch the attached image, please.

Explanation:

To complete the Lewis structure for this covalent compound, you have to draw all the atoms with their valence electrons.

The drew has the nitrogen in the center and the fluoride and oxygen in the sides.

Each one of these atoms has to complete the octet rule, which is the ruler who says that all the atoms want to reach to have eight electrons to feel "stable".

For that reason, you have to arrange the atoms to comply with this rule.

3 0
3 years ago
You mix 265.0 mL of 1.20 M lead(II) nitrate with 293 mL of 1.55 M potassium iodide. The lead(II) iodide is insoluble. What amoun
slava [35]

Answer:

105 grams PbI₂

Explanation:

Pb(NO₃)₂ + 2KI => 2KNO₃ + PbI₂(s)

moles Pb(NO₃)₂ = 0.265L(1.2M) = 0.318 mole

moles KI = 0.293(1.55M) = 0.454 mole => Limiting Reactant

moles PbI₂ from mole KI in excess Pb(NO₃)₂ = 1/2(0.454 mole) = 0.227 mol PbI₂

grams PbI₂ = 0.227 mol PbI₂ x 461 g/mole = 104.68 g ≈ 105 g PbI₂(s)

7 0
3 years ago
Read 2 more answers
. What elements are present in the following chemical formula?<br>KNO3​
White raven [17]
The answer would be potassium nitrate.
8 0
3 years ago
Whose model was discarded as a result of Rutherford's model?
LuckyWell [14K]

Answer:

<u>A. Dalton's</u><u> </u><u>model</u>

Explanation:

Dalton's model was discarded as a result of Rutherford's model.

7 0
3 years ago
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A bottle with a mass of 6.8 g has 23.1 mL of a liquid placed in it. The combined mass of the bottle and the liquid is now 48.8 g
Umnica [9.8K]

Answer:

d = 1.8 g/mL

Explanation:

Given data:

Mass of bottle = 6.8 g

Volume of liquid = 23.1 mL

Mass of bottle + liquid = 48.8 g

Density of liquid = ?

Solution:

First of all we will calculate the mass of liquid.

Mass of liquid = combined mass - mass of bottle

Mass of liquid = 48.8 g - 6.8 g

Mass of liquid = 42 g

Density of liquid:

d = m/v

d = 42 g/ 23.1 mL

d = 1.8 g/mL

5 0
2 years ago
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