For the reaction N2O4(g)⇌2NO2(g), ΔH0=+57.2kJmol−1 and KP=0.113 at 298 K
1) What is KP at 0∘C
2) At what temperature will KP= 1.00?
1) What is KP at 0∘C
Given that K1= 0.113
K2=?
T1= 298 K
T2= 0∘C or 273 K
delta H= =+57.2kJmol−1 or 57200 J / mole
R= 8.314 (gas constant)
ln(K2/K1 )=dH /R (1/t1-1/ t2)
ln(x/0.113)=57200/8.314(1/298-1/273)
then;
ln(x/0.113)= -2.114
x/0.113= 0.1207.
to solve for x which is 0.014
2) At what temperature will KP= 1.00
K1= 1.00
K2=0.113
T1= x
T2= 298 K
delta H= 57200
R= 8.314 (gas constant)
ln(0.113/1.00)=57200/8.314(1/x-1/298)
-2.18=6880/x-23.087
X= 330 K
OR 57 c
Get Answers For Free
Most questions answered within 1 hours.