When ammonia reacts with dinitrogen oxide gas (ΔHf° = 82.05 kJ/mol), liquid water and nitrogen gas are formed. How much heat (in kJ) is liberated or absorbed by the reaction that produces 365 mL of nitrogen gas at 25°C and 743 mm Hg?   ΔHf° (kJ/mol) NH3(g) –46.1 H2O(l) –285.8 N2(g) 0 N2O(g) 82.05

What is the AH°rxn for the reaction of gaseous ammonia and oxygen gas to form gaseous nitrogen monoxide and water vapor? Use the given standard heats of formation. Write the balanced chemical reaction. AH°; NH3 (g) AH°;02 (g) = 0 AH°;NO (g) = 103.56 kJ/mol AH°; H20 (g) = -218.42 kJ/mol = -38.17 kJ/mol %3D

The oxidation of glucose, C6H12O6(s), is described by the following thermochemical equation:C6H12O6(s) + 6 O2(g) → 6 CO2(g) + 6 H2O(l) ΔH = -2772 kJHow much heat, in kilojoules, can be produced by the oxidation of 3.56 g of fuel C6H12O6?Molar mass of C6H12O6 = 180.156 g/mol

A bomb calorimeter, or a constant volume calorimeter, is a device often used to determine the heat of combustion of fuels and the energy content of foods.   In an experiment, a 1.4710 g sample of maleic acid (C4H4O4) is burned completely in a bomb calorimeter. The calorimeter is surrounded by 1159 g of water. During the combustion the temperature increases from 22.46 to 25.59 °C.   The heat capacity of the calorimeter, not including the surrounding water, was determined in a previous experiment to be 852.2 J/°C.   Assuming that no energy is lost to the surroundings, calculate the molar heat of combustion of maleic acid based on these data.   Assuming that no energy is lost to the surroundings, what is the molar heat of combustion of maleic acid, based on these data? (in kJ/mol).   C4H4O4(s) + 3O2(g) → 2 H2O(l) + 4 CO2(g) + Energy