KALTIM.03.00237 

AYO BERLATIH INTERMEDIATE 1 Tahun 2024

SOAL AYO BERLATIH INTERMEDIATE 1 JENJANG SMA

A-AA+01 : 18 : 18

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Sampai saat ini, suka atau tidak, penggunaan bahan bakar fosil masih dominan secara global. Cadangan bahan bakar fosil, terutama yang bersumber dari minyak bumi, diprediksi akan semakin menipis seiring berjalannya waktu. Hal ini menjadi kekhawatiran tersendiri, karena dapat menyebabkan krisis energi jika tidak diantisipasi. Oleh karena itu, selama beberapa dekade terakhir dilakukan upaya untuk mencari dan memanfaatkan sumber bahan bakar alternatif, seperti bioetanol, biodiesel, biomassa metana (biogas), dan hidrogen (*hydrogen fuel*). Tabel berikut menunjukkan komponen senyawa kimia yang terdapat pada beberapa bahan bakar:

Selain *hydrogen fuel*, umumnya bahan bakar yang tercantum dalam tabel tersebut memiliki komponen utama hidrokarbon atau turunannya. Pembakaran sempurna hidrokarbon akan menghasilkan gas karbon dioksida dan uap air, disertai dengan pelepasan energi.Jika diasumsikan bensin hanya mengandung isooktana, maka ketika 57 g bensin dicampur dengan 32 g oksigen dan percikan api dialirkan pada campuran tersebut sehingga terbakar. Berapa gram massa CO2 yang dihasilkan?

*Catatan: Jawaban ditulis dalam bentuk angka tanpa satuan*

**TULIS JAWABAN DI BAWAH :**

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To solve this problem, we need to use the stoichiometry of the combustion reaction of isooctane (\(\text{C}_8\text{H}_{18}\)) with oxygen (\(\text{O}_2\)) to find the mass of carbon dioxide (\(\text{CO}_2\)) produced.

### Step 1: Write the balanced chemical equation for the combustion of isooctane.

The combustion of isooctane (\(\text{C}_8\text{H}_{18}\)) in oxygen (\(\text{O}_2\)) can be represented by the following equation:

\[
\text{C}_8\text{H}_{18} + \text{O}_2 \rightarrow \text{CO}_2 + \text{H}_2\text{O}
\]

First, balance the carbon (C) atoms:

\[
\text{C}_8\text{H}_{18} + \text{O}_2 \rightarrow 8\text{CO}_2 + \text{H}_2\text{O}
\]

Next, balance the hydrogen (H) atoms:

\[
\text{C}_8\text{H}_{18} + \text{O}_2 \rightarrow 8\text{CO}_2 + 9\text{H}_2\text{O}
\]

Finally, balance the oxygen (O) atoms:

\[
\text{C}_8\text{H}_{18} + \frac{25}{2}\text{O}_2 \rightarrow 8\text{CO}_2 + 9\text{H}_2\text{O}
\]

To avoid fractions, multiply the entire equation by 2:

\[
2\text{C}_8\text{H}_{18} + 25\text{O}_2 \rightarrow 16\text{CO}_2 + 18\text{H}_2\text{O}
\]

### Step 2: Calculate the molar masses of isooctane and oxygen.

- Molar mass of \(\text{C}_8\text{H}_{18}\): \(8 \times 12.01 + 18 \times 1.01 = 114.23 \, \text{g/mol}\)
- Molar mass of \(\text{O}_2\): \(2 \times 16.00 = 32.00 \, \text{g/mol}\)

### Step 3: Determine the limiting reactant.

Given:
- Mass of \(\text{C}_8\text{H}_{18}\) (isooctane) = 57 g
- Mass of \(\text{O}_2\) = 32 g

First, find the moles of each reactant:

- Moles of \(\text{C}_8\text{H}_{18}\): 
\[
\frac{57 \, \text{g}}{114.23 \, \text{g/mol}} \approx 0.499 \, \text{mol}
\]
- Moles of \(\text{O}_2\): 
\[
\frac{32 \, \text{g}}{32.00 \, \text{g/mol}} = 1.00 \, \text{mol}
\]

According to the balanced equation, 2 moles of \(\text{C}_8\text{H}_{18}\) require 25 moles of \(\text{O}_2\). The molar ratio of \(\text{C}_8\text{H}_{18}\) to \(\text{O}_2\) is \( \frac{2}{25} \).

Now compare the moles:

\[
\frac{0.499 \, \text{mol} \, \text{C}_8\text{H}_{18}}{1.00 \, \text{mol} \, \text{O}_2}} = \frac{2}{25} \approx 0.08
\]

Since \(0.08\) is greater than \(0.08\), \(\text{O}_2\) is the limiting reactant.

### Step 4: Calculate the amount of \(\text{CO}_2\) produced.

From the balanced equation, 25 moles of \(\text{O}_2\) produce 16 moles of \(\text{CO}_2\).

\[
\text{Moles of CO}_2 = \left(\frac{16}{25}\right) \times \text{moles of } \text{O}_2 = \left(\frac{16}{25}\right) \times 1.00 \, \text{mol} = 0.64 \, \text{mol}
\]

### Step 5: Calculate the mass of \(\text{CO}_2\) produced.

Molar mass of \(\text{CO}_2\) is \(12.01 + 2 \times 16.00 = 44.01 \, \text{g/mol}\).

Mass of \(\text{CO}_2\):

\[
\text{Mass of CO}_2 = 0.64 \, \text{mol} \times 44.01 \, \text{g/mol} \approx 28.17 \, \text{g}
\]

### Final Answer:

The mass of \(\text{CO}_2\) produced is **28** (rounded to the nearest whole number).

Would you like a detailed explanation on any specific step? Here are some related questions you might find interesting:

1. How do you determine the limiting reactant in a chemical reaction?
2. What is the significance of balancing chemical equations?
3. How does the combustion of hydrocarbons impact the environment?
4. What are alternative fuels, and how do they compare with fossil fuels?
5. Can the principles of stoichiometry be applied to industrial processes?

**Tip:** Always double-check the stoichiometric coefficients when solving chemical reaction problems to ensure accuracy.

Learn how to calculate the mass of carbon dioxide produced in the combustion reaction of isooctane with oxygen. This problem involves stoichiometry and molar mass calculations. Suitable for high school chemistry students.

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