The meals-ready-to-eat (MREs) in the military can be heated on a flameless heater. You can purchase a similar product called "Heater Meals." Just pour water into the heater unit, wait a few minutes, and you have a hot meal. The source of energy in the heater is Mg(s) + 2 H₂O(l) → Mg(OH)2 (s) + H₂(g) Calculate the enthalpy change under standard conditions, in joules, for this reaction. What quantity of magnesium is needed to supply the energy required to warm 45 mL of water (d = 1.00 g/mL) from 20. °C to 95 °C? The specific heat capacity of water is 4.184 J/g °C. A, H* (kJ/mol) Compound Mg(OH)2 (s) H₂O(l) -924.54 -285.83 AFER MEALD The "heater meal" uses the reaction of magnesium with water as a source of energy as heat. Enthalpy change = J/mol-rxn g Mg

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 0.7090 g sample of adipic acid (C6H1004) is burned completely in a bomb calorimeter. The calorimeter is surrounded by 1.201×10° g of water. During the combustion the temperature increases from 22.33 to 24.58 °C. The heat capacity of water is 4.184 J gloc!. The heat capacity of the calorimeter was determined in a previous experiment to be 799.0 J/°C. Assuming that no energy is lost to the surroundings, calculate the molar heat of combustion of adipic acid based on these data. CGH1004(s) + (13/2) O2(g) → 5 H,O(1) + 6 CO2(g) + Energy Molar Heat of Combustion = kJ/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

The combustion of titanium with oxygen produces titanium(IV) oxide: Ti(s)+O2(g)→TiO2(g) When 2.060 g of titanium is combusted in a calorimeter, the temperature of the calorimeter increases from 25.00°C to 91.60 °C. If the heat capacity of the calorimeter is 9.84 kJ/°C, what is the heat associated with the combustion of one mole of Ti in this calorimeter?