[tex]\[
CH_{4(g)} + 2O_{2(g)} \rightarrow CO_{2(g)} + 2H_2O_{(l)}: \Delta H = -890 \, \text{kJ}
\][/tex]

Which statement about this reaction is correct?

A. The reaction of one mole of oxygen [tex]$\left( O_2 \right)$[/tex] absorbs [tex]$445 \, \text{kJ}$[/tex] of energy.
B. The reaction of one mole of oxygen [tex]$\left( O_2 \right)$[/tex] releases [tex]$445 \, \text{kJ}$[/tex] of energy.
C. The reaction of one mole of methane [tex]$\left( CH_4 \right)$[/tex] absorbs [tex]$890 \, \text{kJ}$[/tex] of energy.
D. The reaction of two moles of methane [tex]$\left( CH_4 \right)$[/tex] releases [tex]$890 \, \text{kJ}$[/tex] of energy.

Question

29-06-2024
Chemistry

Answered

[tex]\[
CH_{4(g)} + 2O_{2(g)} \rightarrow CO_{2(g)} + 2H_2O_{(l)}: \Delta H = -890 \, \text{kJ}
\][/tex]

Which statement about this reaction is correct?

A. The reaction of one mole of oxygen [tex]$\left( O_2 \right)$[/tex] absorbs [tex]$445 \, \text{kJ}$[/tex] of energy.
B. The reaction of one mole of oxygen [tex]$\left( O_2 \right)$[/tex] releases [tex]$445 \, \text{kJ}$[/tex] of energy.
C. The reaction of one mole of methane [tex]$\left( CH_4 \right)$[/tex] absorbs [tex]$890 \, \text{kJ}$[/tex] of energy.
D. The reaction of two moles of methane [tex]$\left( CH_4 \right)$[/tex] releases [tex]$890 \, \text{kJ}$[/tex] of energy.

Answer :

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GinnyAnswer GinnyAnswer · Answer 1 · 2024-06-29T12:29:44-04:00

Let's analyze the reaction step by step to determine which statement is correct.

### The Reaction
The given reaction is:
[tex]\[ \text{CH}_4(\text{g}) + 2 \text{O}_2(\text{g}) \rightarrow \text{CO}_2(\text{g}) + 2 \text{H}_2\text{O}(\text{l}); \Delta H = -890 \text{kJ} \][/tex]

Here, $\Delta H = -890 \text{kJ}$ indicates that 890 kJ of energy is released when one mole of methane ($\text{CH}_4$) reacts with oxygen ($\text{O}_2$). This release of energy signifies that it is an exothermic reaction.

### Interpretation of $\Delta H$
- If $\Delta H$ is negative, the reaction releases energy.
- If $\Delta H$ is positive, the reaction absorbs energy.

For our reaction:
- $\Delta H = -890 \text{kJ}$ means 890 kJ of energy is released for the combustion of one mole of $\text{CH}_4$.

### Moles of Reactants
From the reaction equation:
- One mole of $\text{CH}_4$ reacts with 2 moles of $\text{O}_2$.

### Energy Released per Mole of $\text{O}_2$
Since 890 kJ is released for 2 moles of $\text{O}_2$:

Energy released per mole of $\text{O}_2$ is:
[tex]\[ \frac{-890 \text{kJ}}{2} = -445 \text{kJ} \][/tex]

### Analyzing the Statements

1. The reaction of one mole of oxygen ($\text{O}_2$) absorbs 445 kJ of energy.
- Incorrect. The negative $\Delta H$ denotes release of energy, not absorption.

2. The reaction of one mole of oxygen ($\text{O}_2$) releases 445 kJ of energy.
- Correct. Each mole of $\text{O}_2$ releases 445 kJ of energy.

3. The reaction of one mole of methane ($\text{CH}_4$) absorbs 890 kJ of energy.
- Incorrect. The reaction releases 890 kJ of energy, not absorbs.

4. The reaction of two moles of methane ($\text{CH}_4$) releases 890 kJ of energy.
- Incorrect. The reaction specifies that one mole of $\text{CH}_4$ releases 890 kJ of energy.

Thus, the correct statement is:
2. The reaction of one mole of oxygen ([tex]$\text{O}_2$[/tex]) releases 445 kJ of energy.