The equilibrium constant of the reaction is 0.323.
Equilibrium constant:
It is expressed as the ratio of concentration of the products to the concentration of reactants. It is represented by K.
The relationship of K with G (Gibbs free energy) is expressed as:
G° = -RTlnK
Here R is the gas constant, T is the temperature.
Calculations:
Convert 25°C to K.
25°C = (25 + 273.15) K
= 298.15 K
Substitute the values in the above expression.
2.8 x 1000 J/mol = -8.314 J/mol.K x 298.15 K x ln(K)
lnK = 2800 J/mol/(-8.314 J/mol.K x 298.15 K)
lnK = -1.13
K = e^-1.13
= 0.323
Learn more about Gibbs free energy here:
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(P1V1=nRT1)/(P2V2=nRT2)
Constant temperature → (P1V1)/(P2V2)
688 mm Hg → 0.905 atm
994 mm Hg → 1.30789 atm
500.2 mL → 0.5002 L
(P1V1)/(P2V2)
(0.905)V1/(1.30789)(0.5002)
V1 = 0.72288 L → 722.88 mL
Models are used to study atoms because we can't exactly study an atom with the naked eye, Using an enlarged model of an atom easier to study because we can pin point the different characteristics of the atom.