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Nat2105 [25]
2 years ago
7

Use the ball and stick models above. If you had a gram of water and a gram of

Chemistry
1 answer:
Sladkaya [172]2 years ago
6 0

Answer:

When the weather is nice, many people begin to work on their yards and homes. For many projects, sand is needed as a foundation for a walk or to add to other materials. You could order up twenty million grains of sand and have people really stare at you. You could order by the pound, but that takes a lot of time weighing out. The best bet is to order by the yard, meaning a cubic yard. The loader can easily scoop up what you need and put it directly in your truck.

Avogadro’s Number

It certainly is easy to count bananas or to count elephants (as long as you stay out of their way). However, you would be counting grains of sugar from your sugar canister for a long, long time. Atoms and molecules are extremely small – far, far smaller than grains of sugar. Counting atoms or molecules is not only unwise, it is absolutely impossible. One drop of water contains about 10 22 molecules of water. If you counted 10 molecules every second for 50 years without stopping you would have counted only 1.6 × 10 10 molecules. Put another way, at that counting rate, it would take you over 30 trillion years to count the water molecules in one tiny drop.

Explanation:

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27.4 g of Aluminum nitrite and 169.9 g of ammonium chloride react to form aluminum chloride, nitrogen, and water. How many grams
GarryVolchara [31]

<u>Answer:</u> The mass of excess reagent (ammonium chloride) remained after the reaction is 62.7 grams

<u>Explanation:</u>

To calculate the number of moles, we use the equation:

\text{Number of moles}=\frac{\text{Given mass}}{\text{Molar mass}}      .....(1)

  • <u>For aluminium nitrite:</u>

Given mass of aluminium nitrite = 27.4 g

Molar mass of aluminium nitrite = 41 g/mol

Putting values in equation 1, we get:

\text{Moles of aluminium nitrite}=\frac{27.4g}{41g/mol}=0.668mol

  • <u>For ammonium chloride:</u>

Given mass of ammonium chloride = 169.9 g

Molar mass of ammonium chloride = 53.5 g/mol

Putting values in equation 1, we get:

\text{Moles of ammonium chloride}=\frac{169.9g}{53.5g/mol}=3.176mol

The chemical equation for the reaction of aluminium nitrite and ammonium chloride follows:

Al(NO_2)_3+3NH_4Cl\rightarrow AlCl_3+3N_2+6H_2O

By Stoichiometry of the reaction:

1 mole of aluminium nitrite reacts with 3 moles of ammonium chloride

So, 0.668 moles of aluminium nitrite will react with = \frac{3}{1}\times 0.668=2.004mol of ammonium chloride.

As, given amount of ammonium chloride is more than the required amount. So, it is considered as an excess reagent.

Thus, aluminium nitrite is considered as a limiting reagent because it limits the formation of product.

Excess moles of ammonium chloride = (3.176 - 2.004) mol = 1.172 moles

Calculating the mass of ammonium chloride by using equation 1, we get:

Excess moles of ammonium chloride = 1.172 moles

Molar mass of ammonium chloride = 53.5 g/mol

Putting values in equation 1, we get:

1.172mol=\frac{\text{Mass of ammonium chloride}}{53.5g/mol}\\\\\text{Mass of ammonium chloride}=(1.172mol\times 53.5g/mol)=62.7g

Hence, the mass of excess reagent (ammonium chloride) remained after the reaction is 62.7 grams

3 0
3 years ago
The number of oxygen atoms in 48.0g of oxygen gas
Doss [256]

Answer:

Now u have 48 g of O2. There. Fore mole=weight/M. W. Of oxygen. Therefor 3mole.

After that if we to multiply the avogadro number with it. So 3 *NA

Now u want only atom calculation then we have 2 molecule of oxygen then multiply it with 2 too.

So final claculation is =3*2*NA.

Explanation:

your welcome

brainlest PLEASEEEEEEE!

3 0
3 years ago
The Ksp of calcium carbonate in water at 25 °C is 2.25 x 10-8. CaCO3(s) &lt;----&gt; Ca2+ (aq) + CO3 2- (aq) What is favored at
seraphim [82]

Answer:

the solubility of CaCO3 is 0.015g/l 25 °C

is favored at equilibrium

Explanation:

The Ksp of calcium carbonate in water at 25 °C is 2.25 x 10-8. CaCO3(s) <----> Ca2+ (aq) + CO3 2- (aq) What is favored at equilibrium?

solubility is the property of a solute to dissolve in a solvent(liquid, gas ) to form a solution(soution can be saturated ,unsaturated, or supersaturated)

CaCO3(s) <----> Ca2+ (aq) + CO3 2- (aq)

in partial dissociation , we can say

2.25x 10^-8=Ca^{2+} +CO^{2-}_{3} }

let Ca^2+=CO3^-2=S

2.25x10^-8=S*S

S^2=2.25x10^-8

S=0.00015mol/L

Converting that to g/l

the relative molecular mass of CaCO3=100g/mol

0.00015*100g/mol

0.015g/l

the solubility of CaCO3 is 0.015g/l @room temperature

is favored   at equilibrium

5 0
3 years ago
A compound has the percent composition 47.40% Pd, 28.50% O, 21.40% C, and 2.69% H. Based on this information, which molecular fo
Helga [31]

Answer:

Pd(O₂CCH₃)₂

Explanation

5 0
3 years ago
Read 2 more answers
In calcium fluoride, what is the closets noble gas that each ion becomes?
alekssr [168]
Calcium fluoride: CaF₂
Ca(2+) >>> Ar (argon)
F(-) >>> Ne (neon)
4 0
3 years ago
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