A 0.600 g sample of tristearin (C57H11O6), a common fat, is combusted in a bomb calorimeter containing 750.0 g of water. The heat capacity of the calorimeter is 326 J/K.  The initial temperature is 19.5 °C. It is known that the heat of combustion of tristearin is -38.0 kJ/g. The specific heat capacity of water is 4.184 J/g.K. (a) How much heat (in kJ) is released by this reaction?   (b) What is the final temperature (in °C)?

[11] A 10.00 g sample of a metal alloy was heated to 88.99 °C. It is then quickly dropped into 40.0 g of water in a calorimeter. The water temperature rises from 19.73 °C to 24.23 °C. Calculate the specific heat of the alloy. [Specific Heat of Water = 4.184 J/g °C and Heat Capacity of Calorimeter = 12.6 J/°C]

A 32.1 g piece of aluminum (which has a molar heat capacity of 24.03 J/°C·mol) is heated to 82.4°C and dropped into a calorimeter containing water (specific heat capacity of water is 4.18 J/g°C) initially at 22.3°C. The final temperature of the water is 25.8°C. Calculate the mass of water in the calorimeter.

A student runs two experiments with a constant-volume "bomb" calorimeter containing 1400. g of water (see sketch at right). First, a 5.000 g tablet of benzoic acid (CH-CO₂H) is put into the "bomb" and burned completely in an excess of oxygen. (Benzoic acid is known to have a heat of combustion of 26.454 kJ/g.) The temperature of the water is observed to rise from 21.00 °C to 42.00 °C over a time of 8.5 minutes. Next, 5.190 g of ethylene (C₂H4) are put into the "bomb" and similarly completely burned in an excess of oxygen. This time the temperature of the water rises from 21.00 °C to 63.35 °C. Use this information, and any other information you need from the ALEKS Data resource, to answer the questions below about this reaction: Is this reaction exothermic, endothermic, or neither? If you said the reaction was exothermic or endothermic, calculate the amount of heat that was released or absorbed by the reaction in the second experiment. exothermic C₂H₂(g) + 30₂(g) → 2CO₂(g) + 2H₂O(g) Be…

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A 47.70 mL volume of 1.00 M HCl was mixed with 47.30 mL of 2.00 M NaOH in a coffee cup calorimeter (with calorimeter constant = 25.0 J/°C) at 21.71 °C. The final temperature of the aqueous solution after the reaction was 29.73 °C. Assuming that them heat capacity of the solution is 4.18 J/g/°C, calculate the following:  The enthalpy change (∆H) for the neutralization in kJ/mol HCl ( this should be a negative number) in kJ/mol HCl