Chemistry

• r= rate
• m= molar masses of each gas

• PV = k
• or 
• P₁V₁ = P₂V₂

moles and temperature are constant (isothermal)

• 
• or
• 

X = mols of species/total moles

n = number of monovalent particles produced

Q_c

same as equilibrium constant

• positive change in enthalpy - endothermic
• negative change in enthalpy - exothermic

ΔH^o_rxn = 

Same reaction for standard enthalpy and gibbs free energy of a reaction

ΔH(reactants to products) + ΔH(products to reactants

for all state functions

positive change in free energy - nonspontaneous

negative change in free energy - spontaneous

higher equilibrium constant = more negative change in free energy = more spontaneous