released (absolute value) when 0.700 kg of liquid ethanol is burned in excess oxygen to make carbon dioxide and liquid water. The enthalpies of formation of the products and reactants are: CO2(g): -393.51 kJ/mol H2O(l): -285.83 kJ/mol O2(g): 0 kJ/mol

When 15.0 mL of 3.00 M NaOH was mixed in a calorimeter with 12.5 mL of 3.00 M HCl, both initially at room temperature (22.0 °C), the temperature increased to 29.0 °C. The resultant salt solution had a mass of 27.50 g and a specific heat capacity of 3.74 J K-1 g-1. What is the heat capacity of the calorimeter (in J/°C)? Note: the molar enthalpy of neutralization per mol is -55.84 kJ mol-1

An experiment was performed to calculate the heat of solution for potassium fluoride. Use the following data to determine its heat of solution. Assume that the specific heat capacity of the solution produced is the same as that of water, 4.184 J⁄g·°C. Identity of Salt   KF Mass of water in calorimeter (g)   52.42 Mass of salt sample (g)   7.32 Initial temperature of Calorimeter (°C)   20.8 Final temperature of Calorimeter (°C)   30.3 Report your answer in kJ/mol to 3 significant figures.

A scientist measures the standard enthalpy change for the following reaction to be 6.7 kJ : CO(g) + H,O(1)–CO;{g) + H2(g) Based on this value and the standard enthalpies of formation for the other substances, the standard enthalpy of formation of CO(g) is kJ/mol.