Mothballs are composed primarily of the hydrocarbon naphthalene (C10H8). When 1.025 g of naphthalene is burned in a bomb calorimeter, the temperature rises from 24.25 ∘C to 32.33 ∘C. Find ΔErxn for the combustion of naphthalene. The heat capacity of the calorimeter, determined in a separate experiment, is 5.11kJ/∘C .

A chemist wastes a delicious brownie by burning it in a bomb calorimeter.  Before burning, the brownie weighed 21.80 grams. During the combustion process in the bomb calorimeter, the heat of the calorimeter increased by 7.87 ∘C.   The known heat capacity of the calorimeter that was used was 42.73 kJ/∘C.  What is the energy content, in kJ/g, of this brownie? (Enter your answer with no units.  Since we are describing the energy content of the brownie, please ENTER THIS NUMBER AS A POSITIVE NUMBER, not a negative number!)

A particular container holds 3.77 mol of neon gas. The volume of this container can be altered by sliding a piston in or out. The volume is changed from 8.60 L to 12.20 L while at the same time the temperature is changed from 303 K to 345 K. The molar heat capacity, Cym, for neon is 12.47 J/(mol · K). Assume that this value will not change over the given temperature range. What is the change in entropy for the gas? AS = J/K TOOLS x10 MacBook Pro

A chemist carefully measures the amount of heat needed to raise the temperature of a 0.88 kg sample of C,H0, from 35.8 °C to 51.4 °C. The experiment shows that 2.34 × 10* J of heat are needed. What can the chemist report for the molar heat capacity of C,H00,? Round your answer to 2 significant digits. |J-mol 1 - 1 •K х10

The combustion of 1.880 g of sucrose, C,H,,O, (s), in a bomb calorimeter with a heat capacity of 4.30 kJ/°C results in an increase in the temperature of the calorimeter and its contents from 22.31 °C to 29.52 °C. What is the internal energy change, AU, for the combustion of 1.880 g of sucrose? AU = kJ Calculate the enthalpy of combustion, AHe, of sucrose in kilojoules per mole. kJ/mol AH. = A étv w MacBook Air DI DD 80 888 F12 F11 F9 F10 F7 FB 3 F4 F5 F6

5. The molar mass of enthalpy of combustion of glucose, C6H1206 is -2803 kJ. A mass of 1.00 g glucose is combusted in a bomb calorimeter. If the calorimeter contains 875 g H20 and the bomb has a heat capacity of 475 J°C1, what is the temperature increase of the bomb calorimeter? The specific heat capacity of water is 4.184 J K-1 g1 and the molar mass of glucose is 180.2 g mol-1.

A 56.1 g sample of polystyrene, which has a specific heat capacity of 1.880 J-g °C-1 is put into a calorimeter (see sketch at right) that contains 250.0 g of water. The temperature of the water starts off at 24.0 °C. When the temperature of the water stops changing it's 29.8 °C. The pressure remains constant at 1 atm. Calculate the initial temperature of the polystyrene sample. Be sure your answer is rounded to the correct number of significant digits. °C thermometer. insulated container water sample. a calorimeter 區 OU Ar

2) The combustion of 0.25 g sucrose, C1HO11, in a bomb calorimeter causes the temperature to rise from 24.9 to 28.3 °C. If the heat capacity of the calorimeter is 4.90 kJ/°C, calculate the heat of combustion of sucrose in kJ/g.

THERMODYNAMICS: A 1.96 g sample of acetic acid (HC;H3O2) was burned in excess oxygen in a bomb calorimeter. The calorimeter, which alone had a heat capacity of 2.67 kJ/°C, contained 776 g of water. The temperature of the calorimeter and its contents increased from 24.51°C to 27.95°C. What is AH (in kJ) for the combustion per 1.00 mol of acetic acid? MW of acetic acid is 60 g/mol. (Round off the final answer to ONE decimal place) Round your answer to 1 decimal place.

A bomb calorimeter has a heat capacity of 6.067 kJ/°C. A sample of vitamin (C31H4602) has an internal energy (DE) = -2.278 X 104 kJ/mol. When 1.434 g of the vitamin sample are burned in oxygen in the calorimeter, determine the final temperature in °C if the initial temperature is 14.51 °C.