Thermodynamics focuses on energy. Energy is the capacity to do work or to produce heat. Heat is the energy that travels between 2 objects that has a temperature. Enthalpy is used to figure out how much work and heat was removed or added to a system. Enthalpy's symbol is ∆H or delta H.
Loss of temperature for the system
Hess's Law states that no matter which direction the reaction happens in, products to reactants or reactants to products, the total enthalpy change is the sum of both sides of the reaction ∆H
Exothermic or Endothermic
Gain of temperature for the system
Acids are described in 2 ways, a Bronsted-Lowry acid or an Arrhenius acid. A Bronsted-Lowry acid is said to donate a proton,H+.After donating the proton, the acid becomes a conjugated base. A Arrhenius acid is described to produce H+. After producing the H+, the acid reacts with an Arrhenius base and acid-base neutralize.
The q=mc∆t equation is used in thermochemistry to calculate heat energy. q=mc∆t has 4 components q,m,c, and ∆t. c is specific heat capacity. SHC is the amount of heat needed to raise the temperature of 1 gram of a substance by 1 degree(C or F) and is measured by Joules/Grams times Temeprature(*C). m stands for the mass of the substance and is measured by grams. ∆t stands for the difference of temperature(∆t=t-final - t-initial) and is measured by *C. q is the symbol for the heat energy of the system.
∆t X m X c
A reaction can be categorized into 2 reactions, exothermic or endothermic. Exothermic reaction is the reaction that loses heat from inside the system and is released to the surrounding system. Meanwhile, endothermic reaction are the reactions that gain heat from the surrounding system.