CEM 142 Exam 1 With Correct Answers|Verified
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
will this process occur
exothermic (-) and entropy (+) - yes, G will be negative
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
will this process occur
exothermic (-) and entropy (+) - yes, G will be negative
