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Sagot :
Certainly! Here is the detailed, step-by-step solution for calculating the enthalpy change ([tex]\(\Delta H\)[/tex]) for the combustion of the hydrocarbon given the provided data.
### Step 1: Understand the given data
- Heat released ([tex]\(q_{\text{cal}}\)[/tex]) during combustion: 6191.78 Joules.
- Number of moles ([tex]\(n\)[/tex]) of the substance: 0.0019243682 moles.
### Step 2: Formula for Enthalpy change
The enthalpy change [tex]\(\Delta H\)[/tex] in kilojoules per mole ([tex]\(kJ/mol\)[/tex]) can be calculated using the formula:
[tex]\[ \Delta H = \frac{q_{\text{cal}}}{n} \][/tex]
### Step 3: Convert Joules to Kilojoules
Since 1 Joule = 0.001 Kilojoules, we first convert the heat released from Joules to Kilojoules:
[tex]\[ 6191.78 \, \text{J} = 6191.78 \times 0.001 \, \text{kJ} \][/tex]
[tex]\[ 6191.78 \, \text{J} = 6.19178 \, \text{kJ} \][/tex]
### Step 4: Calculate Enthalpy Change in [tex]\(kJ/mol\)[/tex]
Now, we divide the heat released (in [tex]\(kJ\)[/tex]) by the number of moles ([tex]\(n\)[/tex]):
[tex]\[ \Delta H = \frac{6.19178 \, \text{kJ}}{0.0019243682 \, \text{mol}} \][/tex]
[tex]\[ \Delta H = 3217.565 \, \text{kJ/mol} \][/tex]
### Step 5: Determine the sign of the Enthalpy Change
For combustion reactions, the enthalpy change is typically exothermic, so the sign of [tex]\(\Delta H\)[/tex] is negative:
[tex]\[ \Delta H = -3217.565 \, \text{kJ/mol} \][/tex]
### Step 6: Round to Three Significant Figures
Finally, we round the value to three significant figures:
[tex]\[ \Delta H = -3217.565 \approx -3218 \, \text{kJ/mol} \][/tex]
Therefore, the enthalpy change [tex]\(\Delta H\)[/tex] for the combustion of the hydrocarbon is [tex]\(-3217.565 \, kJ / mol\)[/tex], rounded to three significant figures, which is [tex]\(-3218 \, kJ / mol\)[/tex].
### Step 1: Understand the given data
- Heat released ([tex]\(q_{\text{cal}}\)[/tex]) during combustion: 6191.78 Joules.
- Number of moles ([tex]\(n\)[/tex]) of the substance: 0.0019243682 moles.
### Step 2: Formula for Enthalpy change
The enthalpy change [tex]\(\Delta H\)[/tex] in kilojoules per mole ([tex]\(kJ/mol\)[/tex]) can be calculated using the formula:
[tex]\[ \Delta H = \frac{q_{\text{cal}}}{n} \][/tex]
### Step 3: Convert Joules to Kilojoules
Since 1 Joule = 0.001 Kilojoules, we first convert the heat released from Joules to Kilojoules:
[tex]\[ 6191.78 \, \text{J} = 6191.78 \times 0.001 \, \text{kJ} \][/tex]
[tex]\[ 6191.78 \, \text{J} = 6.19178 \, \text{kJ} \][/tex]
### Step 4: Calculate Enthalpy Change in [tex]\(kJ/mol\)[/tex]
Now, we divide the heat released (in [tex]\(kJ\)[/tex]) by the number of moles ([tex]\(n\)[/tex]):
[tex]\[ \Delta H = \frac{6.19178 \, \text{kJ}}{0.0019243682 \, \text{mol}} \][/tex]
[tex]\[ \Delta H = 3217.565 \, \text{kJ/mol} \][/tex]
### Step 5: Determine the sign of the Enthalpy Change
For combustion reactions, the enthalpy change is typically exothermic, so the sign of [tex]\(\Delta H\)[/tex] is negative:
[tex]\[ \Delta H = -3217.565 \, \text{kJ/mol} \][/tex]
### Step 6: Round to Three Significant Figures
Finally, we round the value to three significant figures:
[tex]\[ \Delta H = -3217.565 \approx -3218 \, \text{kJ/mol} \][/tex]
Therefore, the enthalpy change [tex]\(\Delta H\)[/tex] for the combustion of the hydrocarbon is [tex]\(-3217.565 \, kJ / mol\)[/tex], rounded to three significant figures, which is [tex]\(-3218 \, kJ / mol\)[/tex].
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