madey21
Answered

A hydrocarbon reacts with oxygen in a bomb calorimeter containing [tex]$2.00 \, \text{kg}$[/tex] of water. The temperature rises by [tex]$0.658^{\circ} \text{C}$[/tex]. The heat capacity of the dry portion of the calorimeter is [tex]$1050 \, \text{J}/^{\circ} \text{C}$[/tex]. What is the heat of the overall calorimeter in Joules?

[tex]\[
\begin{array}{c}
q _{ \text{cal} } = q _{ \text{H}_2 \text{O} } + q _{ \text{dry} } \\
q _{ \text{cal} } = [?] \, \text{J}
\end{array}
\][/tex]

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Answer :

Let's solve the problem step by step.

### Given Data
1. Mass of water ([tex]\(m_{\text{water}}\)[/tex]): [tex]\(2.00 \, \text{kg}\)[/tex]
2. Temperature change ([tex]\(\Delta T\)[/tex]): [tex]\(0.658 \, ^\circ \text{C}\)[/tex]
3. Heat capacity of the dry portion of the calorimeter ([tex]\(C_{\text{dry}}\)[/tex]): [tex]\(1050 \, \text{J/(ºC)}\)[/tex]
4. Specific heat capacity of water ([tex]\(C_{\text{H}_2\text{O}}\)[/tex]): [tex]\(4184 \, \text{J/(kg} \cdot \,^ \circ \text{C)}\)[/tex]

### Steps to Solve

1. Calculate the heat absorbed by the water ([tex]\(q_{\text{H}_2\text{O}}\)[/tex]):
[tex]\[ q_{\text{H}_2\text{O}} = m_{\text{water}} \times C_{\text{H}_2\text{O}} \times \Delta T \][/tex]
Substituting in the values:
[tex]\[ q_{\text{H}_2\text{O}} = 2.00 \, \text{kg} \times 4184 \, \text{J/(kg} \cdot \,^ \circ \text{C)} \times 0.658\, ^\circ \text{C} \][/tex]
[tex]\[ q_{\text{H}_2\text{O}} = 5506.144 \, \text{J} \][/tex]

2. Calculate the heat absorbed by the dry portion of the calorimeter ([tex]\(q_{\text{dry}}\)[/tex]):
[tex]\[ q_{\text{dry}} = C_{\text{dry}} \times \Delta T \][/tex]
Substituting in the values:
[tex]\[ q_{\text{dry}} = 1050 \, \text{J/(ºC)} \times 0.658\, ^\circ \text{C} \][/tex]
[tex]\[ q_{\text{dry}} = 690.9 \, \text{J} \][/tex]

3. Calculate the total heat absorbed by the calorimeter ([tex]\(q_{\text{cal}}\)[/tex]):
[tex]\[ q_{\text{cal}} = q_{\text{H}_2\text{O}} + q_{\text{dry}} \][/tex]
Substituting in the values:
[tex]\[ q_{\text{cal}} = 5506.144 \, \text{J} + 690.9 \, \text{J} \][/tex]
[tex]\[ q_{\text{cal}} = 6197.044 \, \text{J} \][/tex]

### Conclusion

The heat of the overall calorimeter is [tex]\(\boxed{6197.044 \, \text{J}}\)[/tex].