CEM 142 Exam 1 Latest Version Already Graded A

CEM 142 Exam 1 Latest Version Already Graded A Open system mass/matter as well as energy can flow in and out of the system closed system mass/matter can not flow into the system but energy can flow in and out of the system isolated system nothing can enter or leave the system what is the difference between state and path function State function depend only on the initial and final states but not the path taken while a path function requires multiple steps and proofs to get to the final state what does delta H stand for thermal energy in a system endothermic reaction energy entering the system exothermic reaction energy leaving the system when bonds are being formed energy is released when bonds are being broken energy is required entropy measure of possible arrangements 2nd law of thermodynamics for any change in total energy there much be an increase in entropy what unit is used to show entropy delta S what happens to delta S as you increase more molecules it increases why does energy move from hot to cold because once energy is transferred to equilibrium. there are more possible arrangements what state has the most distinguishable arrangements gas because there are no interactions and its random what has a higher entropy? water freezing or ice melting ice melting because there are more possible arrangements due to more molecules and less interactions does entropy have to increase in the system a process to exist no, it just has to occur in that universe. either system or surroundings how do you calculate Snet total Ssytem + Ssurroundings what has the highest Hvap the molecules with more hydrogen bonds because more energy is need to overcome the IMF's what is the relationship between delta H and T entropy= thermal energy/temperature Gibbs free energy equation ΔG = ΔH - TΔS