Answer:
a=28600J; b=90.6 J/K; c=402 torr
Explanation:
(a) considering the data given
Vapour pressure P1 =0 at Temperature T1 = 42.43˚C,
Vapour pressure P2 = 273.15 at Temperature T2= 315.58 K)
Using the Clausius-Clapeyron Equation
ln (P2/P1) = (ΔH/R)(1/T2 - 1/T1)
In 760/140 = ΔH/8.314 J/mol/K × (1/315.58K -- 1/273.15K)
ΔH vap= +28.6 kJ/mol or 28600J
(b) using the Equation ΔG°=ΔH° - TΔS to solve forΔS.
Since ΔG at boiling point is zero,
ΔS =(ΔH°vap/Τb)
ΔS = 28600 J/315.58 K
= 90.6 J/K
(c) using ln (P2/P1) = (ΔH/R)(1/T2 - 1/T1)
ln P298 K/1 atm = 28600 J/8.314 J/mol/K × (1/298.15K - 1/315.58K)
P298 K = 0.529 atm
= 402 torr
Answer:
An atom is the smallest particle of an element that can take part in a chemical reaction while a molecule is a group of chemically combined atoms.
Explanation:
Answer: Gas , Solid and Liquid
Explanation:
To complete each sentence , One can easily conclude that the various state of matter are in question here.
To further explain better,
(1) Gas molecule is consider to b moving and also move at a faster rate is respect to others.
(2)Solid molecule usual takes a standing still position unless an external pressure acts on it.
(3) Liquid molecule is capable of starting at same location and then move to another location but not at a faster rate compare to gas molecule.
Use Ideal Gas equation since values are given in Pressure (P), Volume (V), Temperature (T).
P V = n R T ; n= PV / RT
You can't use 1 mole= 22.4 L equation. Temperature and pressure values are not standard. ( 1 atm, 0
To choose the value of R ( gas constant), check out the units of other values in the equation. They are in atm,liter, kelvin, and mole. So, its value is 0.082 L atm/ K mol.
P= 0.97 atm
V= 35.83 * 10 ⁻³ L (conversion from ml to, just multiplied by 10 ⁻³ )
R= 0.082 L atm/ K mol
T= (25.3 + 273) K ( recall Kelvin = Celcius + 273; K= °C + 273<span>)
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Substitute values into equation of n= PV / RT
n= (0.97 atm) (35.83 * 10 ⁻³ L) / (0.082 L atm/ K mol) (298.3 K)= 0.014 mole
The answer is 0.014 mole
