How many moles of aluminum are equivalent to 4.816 × 1024 atoms?

How many grams of water are produced from the combustion of 45.2 g of

Zina [86]

Answer:

101.56 of H₂O

Explanation:

The balanced equation for the reaction is given below:

CH₄ + 2O₂ —> CO₂ + 2H₂O

Next, we shall determine the mass of CH₄ that reacted and the mass of H₂O produced from the balanced equation. This is illustrated below:

Molar mass of CH₄ = 12 + (4×1.01)

= 12 + 4.04

= 16.04 g/mol

Mass of CH₄ from the balanced equation = 1 × 16.04 = 16.04 g

Molar mass of H₂O = (2×1.01) + 16

= 2.02 + 16

= 18.02 g/mol

Mass of H₂O from the balanced equation = 2 × 18.02 = 36.04g

SUMMARY:

From the balanced equation above,

16.04 g of CH₄ reacted to produce 36.04 g of H₂O.

Finally, we shall determine the mass of water, H₂O produced by the reaction of 45.2 g of methane, CH₄. This can be obtained as illustrated below:

From the balanced equation above,

16.04 g of CH₄ reacted to produce 36.04 g of H₂O.

Therefore 45.2 g of CH₄ will react to produce = (45.2 × 36.04)/16.04 = 101.56 g of H₂O.

Thus, 101.56 of H₂O were obtained.

7 0

3 years ago

Please help!! A compound with a molar mass of 544.0 g/mol is made up of 26.5 grams Carbon, 2.94 grams

lukranit [14]

Answer:

1. Empirical formula = C₃H₄O₆

2. Molecular formula = C₁₂H₁₆O₂₄

Explanation:

From the question given above, the following data were obtained:

Molar mass of compound = 544 g/mol

Mass of Carbon (C) = 26.5 g

Mass of Hydrogen (H) = 2.94 g

Mass of oxygen (O) = 70.6 g

Empirical formula =?

Molecular formula =?

1. Determination of the empirical formula of the compound.

C = 26.5 g

H = 2.94 g

O = 70.6 g

Divide by their molar mass

C = 26.5 / 12 = 2.208

H = 2.94 / 1 = 2.94

O = 70.6 / 16 = 4.4125

Divide by the smallest

C = 2.208 / 2.208 = 1

H = 2.94 / 2.208 = 1.33

O = 4.4125 / 2.208 = 2

Muitiply through by 3 to express in whole number.

C = 1 × 3 = 3

H = 1.33 × 3 = 4

O = 2 × 3 = 6

Empirical formula = C₃H₄O₆

2. Determination of the molecular formula of the compound.

Molar mass of compound = 544 g/mol

Empirical formula = C₃H₄O₆

Molecular formula = [C₃H₄O₆]ₙ

[C₃H₄O₆]ₙ = 544

[(12×3) + (4×1) + (16×6)]n = 544

[36 + 4 + 96]n = 544

136n = 544

Divide both side by 136

n = 544 / 136

n = 4

Molecular formula = [C₃H₄O₆]ₙ

Molecular formula = [C₃H₄O₆]₄

Molecular formula = C₁₂H₁₆O₂₄

6 0

3 years ago

Read 2 more answers

!!!!!!

Olin [163]

Answer:

0.192 mol N₂O

Explanation:

Step 1: Write the balanced equation

NH₄NO₃(aq) ⇒ N₂O(g) + 2 H₂O(l)

Step 2: Establish the appropriate molar ratio

According to the balanced equation, the molar ratio of NH₄NO₃ to N₂O is 1:1.

Step 3: Calculate the number of moles of N₂O formed upon complete reaction of 0.192 moles of NH₄NO₃

We will use the previously established molar ratio.

0.192 mol NH₄NO₃ × 1 mol N₂O/1 mol NH₄NO₃ = 0.192 mol N₂O

3 0

3 years ago

HELP ASAP!!! 15 POINTS

sergij07 [2.7K]

Green plants absorb some of the sunlights energy

3 0

3 years ago

Read 2 more answers

How many moles of chlorine gas can be produced when 162.3 grams of aluminum chloride decompose ?

Volgvan

Answer: 6.77 x 1022 molecules of Cl2.

Explanation: First you need to write the correct BALANCED chemical reaction equation. Then you can determine how many moles of

C

l

2

would be produced from the available moles of Cl in 10.0g of

A

l

C

l

3

. Finally, you will convert this value into the number of molecules using Avogadro's number.

2

A

l

C

l

3

→

2

A

l

+

3

C

l

2

So, TWO moles of

A

l

C

l

3

will produce THREE moles of

C

l

2

.

The molecular weight of

A

l

C

l

3

is 133.33g/mol, so 10.0g is 10.0/133.33 = 0.075mol

With our equation ratio of 3/2 this will produce 0.1125 mol

C

l

2

.

0.1125 * 6.022 x

10

23

molecules/mole = 6.77 x

10

22

molecules of

C

l

2

4 0

3 years ago