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The temperature of 3.50 kg of water is raised by 1.17 when 1g of hydrazine N2H4 is burned in a bomb calorimeter. The calorimeter has a heat capacity of 883 how much heat is given off by the sample

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The heat given off by the sample is approximately 16842.19 J.

To calculate the heat given off, we can use the formula
\( Q = mc\Delta T \), where Q is the heat, m is the mass, c is the specific heat capacity, and
\( \Delta T \) is the change in temperature.

Given:

- Mass of water (m) = 3.50 kg

- Change in temperature (
\( \Delta T \)) = 1.17 °C

- Specific heat capacity of water (c) ≈ 4186 J/kg°C

- Heat capacity of the calorimeter (
\( C_{\text{calorimeter}} \)) = 883 J/°C


\[ Q_{\text{water}} = m \cdot c \cdot \Delta T = 3.50 \, \text{kg} \cdot 4186 \, \text{J/kg C} \cdot 1.17 \,{^\circ C} \]


\[ Q_{\text{calorimeter}} = C_{\text{calorimeter}} \cdot \Delta T = 883 \, \text{J/ C} \cdot 1.17 \°C} \]

The total heat given off (
\( Q_{\text{total}} \)) is the sum of
\( Q_{\text{water}} \) and \( Q_{\text{calorimeter}} \).


\[ Q_{\text{total}} = Q_{\text{water}} + Q_{\text{calorimeter}} \]


\[ Q_{\text{total}} \approx (3.50 \, \text{kg} \cdot 4186 \, \text{J/kgC} \cdot 1.17 \, \text{C}) + (883 \, \text{J/C} \cdot 1.17 \, \text{C}) \]


\[ Q_{\text{total}} \approx 16842.19 \, \text{J} \]

User Marcelo Velasquez
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