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Chemistry

1 answer:

ser-zykov [4K]3 years ago

8 0

Answer:

I don't know the answer of this question.

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Alkanes are hydrocarbons containing only single bonds. Acyclic alkanes have carbon atoms arranged in chains, whereas cycloalkane

sashaice [31]

Answer:

156 Hydrogen atoms

Explanation:

<u>Any acyclic alkane has a molecular formula that can be expressed as</u>:

CₙH₂ₙ₊₂

Where <em>n</em> is any integer and the number of carbon atoms. For example, Propane has 3 carbon atoms, this means it would have [2*3+2] 8 hydrogen atoms, resulting with a formula of C₃H₈.

An acyclic alkane with 77 carbon atoms would thus have:

2*77 + 2 = 156 hydrogen atoms

4 0

3 years ago

Sulfur trioxide is a gas that reacts with liquid water to produce aqueous sulfuric Acid or acid rain what is the equation for th

bearhunter [10]

Answer:

SO₃(g) + H₂O(l) → H₂SO₄(aq)

Explanation:

The<em> molecular formula for the involved species</em> are:

Sulfur trioxide = SO₃. ("trioxide" indicates the presence of 3 oxygen atoms).

Water = H₂O

Sulfuric acid = H₂SO₄

With the above information in mind we can proceed to write the reaction equation:

SO₃(g) + H₂O(l) → H₂SO₄(aq)

5 0

3 years ago

A sample of octane undergoes combustion according to the equation 2 C8H18 + 25 O2 → 16 CO2 + 18 H2O ΔH°rxn = -11018 kJ. What mas

Anna71 [15]

Answer:

$\large \boxed{\text{528.7 g} }$

Explanation:

It often helps to write the heat as if it were a reactant or a product in the thermochemical equation.

Then you can consider it to be 11018 "moles" of "kJ"

We will need a chemical equation with masses and molar masses, so, let's gather all the information in one place.

M_r: 32.00

2C₈H₁₈ + 25O₂ ⟶ 16CO₂ + 8H₂O + 11 018 kJ

n/mol: 7280

1. Moles of O₂

The molar ratio is 25 mol O₂:11 018 kJ

$\text{Moles of O}_{2} = \text{7280 kJ} \times \dfrac{\text{25 mol O}_{2}}{\text{11 018 kJ}} = \text{16.52 mol O}_{2}$

2. Mass of O₂

$\text{Mass of C$_{8}$H}_{18} = \text{16.52 mol O}_{2} \times \dfrac{\text{32.00 g O}_{2}}{\text{1 mol O}_{2}} = \textbf{528.6 g O}_{2}\\\text{The reaction requires $\large \boxed{\textbf{528.67 g O}_{2}}$}$