We assume the energy released = energy absorbed, so we can find the Enthalpy by finding the energy absorbed by water. ![]() UNDERSTAND ENERGY TRANSFER and how experimental data and lit values fit in for example, the energy released by the molecules is absorbed by the surrounding water, why does it not matter if we use C or K ? c and mass must be in the same units !Ĭ is typically given in J/gC or J/gK or kJ/gC or kJ/kgK EXPLANATION with SAMPLE PROBLEMS (simple) = (mass of substance being heated or cooled) x (SHC of that substance) x ( change in Temp) specific heat capacity(SHC) c is the amount of energy Q needed to raise 1 g* of a substance by 1 C* be able to use Q=mc dT to solve simple problems of pure substances that are heated or cooled Clarification on Standard Enthalpy of Reaction and the Molar Ratios we will look at the energy of reactions = ENTHALPY OF REACTION "c" = specific heat capacity in J/gK (the UNITS are important) ![]() the energy absorbed or released by the surroundings CAN be measured using ![]() ![]() STANDARD ENTHALPY is when you measure the enthalpy at 100 kPa of pressure, and T=298 K The energy a reaction releases or absorbs is the ENTHALPY of Reaction, in kJ/mol. Energy is TRANSFERRED between the molecules in a reaction and its SURROUNDINGS TEMPERATURE is a measure of the AVERAGE KINETIC ENERGY of the particles in a sample
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