Visible light, radio waves, microwave radiation, infrared, ultraviolet radiation, X-rays, and gamma rays all

What is the chemical formula for iron(2) oxide

solmaris [256]

Iron (II) oxide is composed of iron with an oxidation number of +2 (shown by the II after iron) and an oxygen that has an oxidation number of -2 (oxygen almost always has an oxidation state of -2). Since the anion and cation both have a charge of +or- 2, they bond with each other with a 1 to 1 ratio and the formula should be FeO

I hope this helps. Let me know if anything is unclear.

7 0

3 years ago

If you react 2.00 g of hydrogen completely using 15.87 g of oxygen to produce water, how much water (in grams) will you have?

leonid [27]

Answer:

The amount (mass) of water we will have is 17.869 grams

Explanation:

The molar mass of hydrogen gas H₂ = 2.016 grams/mole

The molar mass of oxygen gas = 31.999 g/mol

Therefore, 2.00 g of hydrogen will give;

2.00/2.016 = 0.9921 moles of H₂ gas and

15.87 g of O₂ will give;

15.87/31.999 = 0.49595 moles

The reaction is as follows;

2H₂ (g) + O₂ (g) → 2H₂O (l)

Two moles of H₂ react with one mole of O₂ to produce two moles of H₂O

Therefore 0.9921 moles of H₂ will react with 0.9921/2 or 0.49595 moles of O₂ to produce 0.9921 moles of H₂O

From the above we note that all the H₂ and O₂ are completely consumed to form 0.9921 moles of H₂O

Molar mass of H₂O = 18.01528 g/mol

Number of moles = Mass/(Molar mass)

∴ Mass of H₂O = (Molar mass) × (Number of moles)

= 18.01528 g/mol × 0.9921 moles = 17.869 grams

Therefore the amount (mass) of water we will have = 17.869 grams.

8 0

3 years ago

If 43.7 g of iron is completely used to produce 62.5 g of iron (III) oxide, how many grams of oxygen are involved in the reactio

Kobotan [32]

Mass of Oxygen : 18.8 g

<h3>Further explanation</h3>

Reaction(balanced) :

4Fe + 3O₂ → 2Fe₂O₃

mass Fe = 43.7 g

mol Fe(MW= 55,845 g/mol) :

$\tt mol=\dfrac{mass}{MW}\\\\mol=\dfrac{43.7}{55.845}\\\\mol=0.783$

mol O₂ : mol Fe = 3 : 4, so mol O₂ :

$\tt \dfrac{3}{4}\times 0.783=0.5873$

Mass O₂(MW=32 g/mol) :

$\tt mass=mol\times MW\\\\mass=0.5873\times 32\\\\mass=18.7936~g\approx 18.8$

Or simply you can Conservation of mass, where the masses before and after the reaction are the same

<em>mass reactants=mass products</em>

mass iron+mass oxygen=mass iron (III) oxide

43.7 g + mass oxygen=62.5 g

mass oxygen = 62.5 - 43.7 = 18.8 g

5 0

3 years ago

What mass of CO2 would be generated along with 35.00g of NaCl?

Sunny_sXe [5.5K]

Answer: The quantitative interpretation of the reaction is as follows: 84.01 g (1 mol) of sodium

bicarbonate reacts with 36.46 g (1 mol) of hydrochloric acid to generate 58.44 g (1 mol) of salt,

18.02 g (1 mol) of water, and 44.01 g (or 1 mol) of carbon dioxide. Of course the starting

quantity of NaHCO3 may be more or less than 84.01 g, but a proportionate quantity of the

hydrochloric acid will be consumed, and proportionate quantities of the products will be formed.

For example, should 100.00 g of NaHCO3 react with excess acid, the theoretical mass of salt

produced would be calculated as follows:

58.44 g sodium chloride 100.00 g sodium bicarbonate

84.01 g sodium bicarbonate = 69.55 g sodium

chloride

Note that when a bicarbonate is reacted with excess acid, the salt produced is the only substance

not readily volatile. That is, the unreacted acid, the water, and the carbon dioxide are easily

removed by heating. Does this help?

3 0

3 years ago

What is the product of silver nitrate + lead ii nitrate?

Kisachek [45]

Answer:

Explanation:

In theory, not much of anything. The vast majority of nitrates are water soluble. Aside, not sure what chemistry level you are at but you will probably be asked to know or memorize some solubility rules. This, for lack of a better phrase, Nitrate rule, is near spot on. With one exception—a rare one—all metal cationic nitrates are soluble in water. All of them. So, assuming you are talking about aqueous, water-based solutions of these salts and mixing them together, I expect nothing to occur. Both solutions, I believe are colorless in water and will thus remain so. If you had say a solution of Iron (III) nitrate and copper (II) nitrate, slightly different story. Both are colorful solutions and I would think you might see blending of colors but no reaction; no precipitate will form. You will probably learn about markers of a chemical reaction. One of these is a color change. Note, you should read this as a change of color from what you previously had. Going from red to blue or colorless to colored (or vice versa) is a strong indication of a reaction (e. g. evidence of bond-breaking and bond-formation). The mere mixing of colors does not constitute a chemical reaction.

3 0

3 years ago