SCH4U Thermodynamics. * Energy difference between the reactants and products. ΔH = H products - H reactants As long as pressure remains constant, the.

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SCH4U Thermodynamics

* Energy difference between the reactants and products. ΔH = H products - H reactants As long as pressure remains constant, the enthalpy change of the chemical system is equal to the flow of thermal energy in and out of the system or… ΔH system = l q system l

* The change in bond energy (ΔH) for 1 mole of a substance…

Determine the ΔH combustion for hexane if burning 30g releases 1452kJ. If the combustion of 1 mole of butane releases 2871 kJ, how much heat will be released by the combustion of 13g?

* Determine the enthalpy change ( ΔH ) of a rxn by measuring the energy change ( q ) of the surroundings. The law of conservation of energy: ΔH system = -q surroundings

* To determine the molar enthalpy (ΔH X ) during a reaction: 1.q = mcΔT 2.n = m/M or n = cv 1.ΔH mol = -q/n

* Determine the ΔH combustion for propane if 21 g of propane raises 5g of water by 50°C

* If the ΔH comb si 34.5 kJ/mol and 2.75 mol of the substance are combusted, what is the energy of the rxn?

* Calculate ΔH for Dissolution Reactions: An energy change called enthalpy of solution, ΔH sol, occurs when a substance dissolves in water. A student places 125g of liquid water at 24.2°C into a coffee-cup calorimeter, and then adds 10.5g of solid potassium bromide, KBr(s), also at 24.2°C. He stirs the liquid until the potassium bromide dissolves, and then determines that the temperature has changed to 21.1°C. Calculate the molar enthalpy change for this dissolution reaction, ΔH sol. Assume that the specific heat capacity, c, of the liquid in the calorimeter is the same as the specific heat capacity of water.

Draw potential energy diagrams for each of the following: * CO 2 (s) kJ  CO 2 (g) * CaCl 2 (s)  CaCl 2 (aq) ΔH sol = kJ * 2 Ag (s) + Cl 2 (g)  2 AgCl (s) kJ