1.11g of methane CH4 is burned in a bomb calorimeter containing 1000 grams of water. The initial temperature of water is 24.85 degrees Celsius. The specific heat of water is 4.184 J/g degrees Celsius. The heat capacity of the calorimeter is 695 J/degrees Celsius. After the reaction the final temperature of the water is 35.65 degrees Celsius. Calculate the heat absorbed by the water. Then calculate the heat absorbed by the calorimeter.

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Chemistry

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11 February, 02:13

1.11g of methane CH4 is burned in a bomb calorimeter containing 1000 grams of water. The initial temperature of water is 24.85 degrees Celsius. The specific heat of water is 4.184 J/g degrees Celsius. The heat capacity of the calorimeter is 695 J/degrees Celsius. After the reaction the final temperature of the water is 35.65 degrees Celsius. Calculate the heat absorbed by the water. Then calculate the heat absorbed by the calorimeter.

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Diamond Myers · Answer 1

Given:

M methane = 1.11g CH4

M calories = 1000g or g of H2O

C heat capacity = 4.184 J/g °C of H2O

C heat capacity = 695 J/°C

Ti = 24.85 °C

Tf = 35.65 °C

Ask: ΔH = ?

Formula: q=mCΔT

= (1000 g) (696 J/°C) (10.8°C)

= 7506000 J H2O (endothermic) release heat

q reaction = - q calorimeter

= - 7506000 J = ΔH