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how will increasing pressure affect the following rxn
N2(g)+3H2(g)<--->2NH3
favor forward rxn
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(t/f) increasing the pressure of a system will shift equilibrium so as to increase number of moles produced
false, increase pressure will shift in favor of less moles of gas
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how would increasing temp affect
A<-->B+heat
favor reverse rxn
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isolated system? close system? open system?isothermal process?
- isolated- CAN NOT exchange energy nor matter with surrounding
- closed- CAN NOT exchange matter
- open-CAN exchange both
- isothemal process- under constant temp
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adiatbatic process?
process in which no heat exchange occurs btwn the system and surounding
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formula for calculating heat (q) absorbed or released by a process
- q=mc(delta t)
- m-mass
- c-heat capacity
- t-temp
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formula for delta Hrxn
sum of delta Hf of products -sum of delta Hf of reactants
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whats standard heat of formation (delta Hf)
the enthalpy change that occurs when one mole of a compound is formed from its elements in their standard states.
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bond dissociation energy?
the amount of energy required to break a particular bond in one mole of gaseous molecules
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entropy?
measure of disorder or randomness of a system
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when does a system reach maximum entropy
at its equilibrium
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under what conditions will rxn with + delta H and + delta S be spontaneous?
high temp
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under what conditions will rxn with - delta H and -delta S be spontaneous
low temp
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whats the value of delta G at equilibrium?
0
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standard free energy delta Go
delta G of a process at 25 oC, 1 atm, and 1 M concentration for all reactants
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(t/f) delta Go=-RTlnKeq
true
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(t/f) once the rxn starts
delta G=delta Go+RTlnQ
true
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whats standard pressure in atm, mmHg, torr?
1 atm = 760 mmHg = 760 torr
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Charlie's law
V1/T1=V2/T2
-
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unit of density for gas, and formula
g/L
d=m/V=P(MM)/RT
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in what condition is the ideal gas most corret
low pressure, high temp
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how do actual volume and predicted volume of gas compare at moderately high pressure? extremely high pressure?
moderate- less than predicted
extreme more than predicted
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how do actual volume and ideal volume of a gas compare at very low temp
less than predicted
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Dalton's law of partial pressure
total pressure is sum of partial pressure of each component
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formula for partial pressure of A
- Pa=PtXa
- Xa=mol of A/total mol
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what is effusion
flow of gas particles under pressure from one container to another through a small opening
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(t/f) the rate of effusion for two molecules are directly proportional to the square root of their molar masses.
false, the rate of effusion are inversely proportional, just as in diffusion
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emulsion?
mixture of immisible liquids which are broken up into extremely small particles
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