A 21.8 g sample of ethanol (C2H5OH) is burned in a bomb calorimeter, causing the temperature to rise from 25.0°C to 62.3°C. Given that the molar mass of ethanol is 46.07 g/mol, what is the heat capacity of the calorimeter?

Calculate the caloric content of table sugar (sucrose, C12H22O11), given that the standard enthalpy of formation of sucrose is -2226.1 kJ/mol. For comparison, the standard enthalpy of formation of palmitic acid (C16H32O2), a dietary fat found in beef and butter, is -208 kJ/mol. Use H2O(l) in the balanced chemical equations, as the metabolism of these compounds produces liquid water.

One tablespoon of peanut butter has a mass of 16 g. It is combusted in a calorimeter whose heat capacity is 120.0 kJ/°C. The temperature of the calorimeter rises from 22.2 °C to 25.4 °C. Find the food caloric content of peanut butter.

What is the specific heat capacity of the bomb calorimeter if burning 100.0 moles of sulfamic acid results in a temperature increase of 4.57°C, given that the ΔErn for the combustion of 1 mole of sulfamic acid is -686.2 kJ?

A 2.49 g sample of aniline (C6H5NH2, molar mass = 93.13 g/mol) was combusted in a bomb calorimeter with a heat capacity of 4.25 kJ/°C. If the temperature rose from 29.5 °C to 69.8 °C, determine the value of ΔH°comb for aniline.

A 6.55 g sample of aniline (C6H5NH2, molar mass = 93.13 g/mol) was combusted in a bomb calorimeter with a heat capacity of 14.25 kJ/°C. If the initial temperature was 32.9°C and the combustion of aniline releases 30.0 kJ/g, what is the final temperature of the calorimeter?

A 6.55 g sample of aniline (C6H5NH2, molar mass = 93.13 g/mol) was combusted in a bomb calorimeter. If the temperature rose by 32.9°C, use the information below to determine the heat capacity of the calorimeter. The balanced reaction is: 4 C6H5NH2(l) + 35 O2(g) → 24 CO2(g) + 14 H2O(g) + 4 N2(g). Given that the standard enthalpy of combustion for aniline is -3170 kJ/mol, what is the heat capacity of the calorimeter?

A calorimeter is to be calibrated: 72.55 mL of water at 71.6 °C is added to a calorimeter containing 58.85 mL of water at 22.4 °C. After stirring and waiting for the system to equilibrate, the final temperature reached 47.3 °C. Determine the calorimeter constant, given that the specific heat capacity of water is 4.18 J/g°C.

In a constant-volume calorimetry experiment using a bomb calorimeter, what thermodynamic quantity is directly measured?