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2 years ago

What is the mass of Al₂O3 that will contain 10 kg of aluminium?

Chemistry

2 answers:

Oksanka [162]2 years ago

5 0

Answer:

1 mole of Al2O3 = 102 grams

1 mole of Al2 = 54 grams

102 grams of Al2O3 contains = 54 gram of Al2

10kg of Al2O3 contains = (54/102)*10000g Al2

= 5294.11 g Al2 or 5.29411 kg

fredd [130]2 years ago

4 0

Answer:

108

Explanation:

Molar mass of Al2O3 = (27 × 2) + (16 × 3)

= 54 + 48 = 102 g/mol

Moles in 204 g of Al2O3 = 204 g/(102 g/mol)

2 mol

Mass of aluminum in 1 mol of Al2O3 = 27 g × 2

= 54 g

Mass of aluminum in 2 mol of Al2O3 = 54 g × 2

= 108 g

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Vanyuwa [196]

Answer: Option (D) is the correct answer.

Explanation:

Vapor pressure is defined as the pressure exerted by the vapors which are present on the surface of a liquid.

For example, vapor pressure of water at room temperature is 0.0313 atm.

On the other hand, the temperature at which the vapor pressure of a liquid equals atmospheric pressure is known as boiling point.

For example, boiling point of water at room temperature is $100^{o}C$ .

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3 years ago

How many grams of sodium sulfide can be produced when 45.3 g Na react with 105 g S?

RoseWind [281]

The chemical reaction would be as follows:

2Na + S → Na2S

We are given the amount of the reactants to be used in the reaction. We use these to calculate the amount of product. We do as follows:

45.3 g Na ( 1 mol / 22.99 g ) = 1.97 mol Na
105 g S ( 1 mol / 32.06 g ) = 3.28 mol S

The limiting reactant would be Na. We calculate as follows:

1.97 mol Na ( 1 mol Na2S / 2 mol Na ) (78.04 g / mol ) = 76.87 g Na2S produced

8 0

3 years ago

Do the number of atoms change in a chemical reaction? I will give brainliest

padilas [110]

Answer:

No.

Explanation:

The reason comes the Law of Conservation of Mass.

In an ordinary chemical reaction, you cannot create or destroy atoms.

So, you must have as many atoms at the beginning of a reaction (in the reactants) as at the end (in the products)

We use this principle to balance chemical equations.

For example, the equation for the formation of water from hydrogen and oxygen is

2H₂ + O₂ ⟶ 2H₂O

There are four atoms of H and two of O both before and after the reaction.

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3 years ago

Determine the molarity of a 6.0 mole% sulfuric acid solution with SG-a 1.07 Note: Atomic Weight: S (32), O 16); H (O)

marin [14]

Answer:

The molarity of a 6.0 mole% sulfuric acid solution is 2.8157 Molar.

Explanation:

Suppose there are 100 moles in solution:

Moles of sulfuric acid = 6% of 100 moles = 6 moles

Mass of 6 moles of sulfuric acid = 6 mol × 98 g/mol=588 g

Moles of water = 100%- 6% = 94%= 94 moles

Mass of water = 94 mol × 18 g/mol = 1692 g

Specific gravity of the solution ,S.G= 1.07

Density of solution = D

$S.G=\frac{D}{d_w}$

$d_w$ = density of water = 1 g/mL

$D=S.G\times d_w=1.07\times 1 g/mL=1.07 g/mL$

Mass of the solution = 588 g + 1692 g = 2280 g

Volume of the solution = V

Volume = $\frac{Mass}{Density}$

$=\frac{2280 g}{1.07 g/mL}=2130.84 mL=2.13084 L$

1 mL = 0.001 L

$Molarity = \frac{n}{V(L)}$

n = number of moles of compound

V = volume of the solution in L

here we have ,n = 6 moles of sulfuric acid

V = 2.13084 L

So, the molarity of the solution is :

$Molarity=\frac{6 mol}{2.13084 L}=2.8157 mol/L$

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3 years ago

Tartaric acid, h2c4h4o6, has two acidic hydrogens. the acid is often present in wines and precipitates from solution as the wine

chubhunter [2.5K]

Balance Chemical equation:

C4H6O6 + 2NaOH ⇒ Na2C4H4O6 + 2H2O

Given Data:

Molarity of NaOH =0.3000

Vol. of NaOH = 21.65

Solution:

moles of NaOH = (0.3000 × 21.65)÷1000 = 0.0064 mol

According to balance chemical equation

NaOH : C4H6O6

2 : 1

0.0064 = (1/2) ×0.0064 = 0.0032 mol

So these 0.0032 mol of tartaric acid are prsent in 50.0 ml of solution.

So in I littre of solutions, its concentration will be as follow

M = 0.0032 × 1000/50 = 0.064 M

Result:

The concentration of acid will be 0.064 M.

8 0

3 years ago

What is the mass of Al₂O3 that will contain 10 kg of aluminium?​

What is the mass of Al₂O3 that will contain 10 kg of aluminium?