Nitrosyl chloride (NOCl) decomposes at high temperature. The equation is
2 NOCl (g) -> 2 NO (g) + Cl2 (g) at 227C
Using delta H = 81.2 kJ and delta S = 128 J/K, calculate the value of the equilibrium constant for this reaction.
a 1.60 X 10-2
b. 2.1 X 10-7
c. 62.8
d. 4.9 X 106
e. 3,20 X 109
help no idea?
dGo = dH - TdS
Subwstitute T, dS, and dH and solve for dG. Then dG = -RTlnK
Solve for K.
Don't forget that dH has units of kJ/mol and dS has units of J/mol.
the new delta s= .128
81.2-(227x.128)=52.144
52.144=-rtlnk
what is rt?
R is 0.08206 just like in PV = nRT.
T is listed in the problem as 227 C (which must be converted to kelvin).
still not getting ans
Show your work.
To calculate the value of the equilibrium constant (K) for the given reaction, we can use the equation:
ΔG = ΔH - TΔS
Where ΔG is the change in Gibbs free energy, ΔH is the change in enthalpy, ΔS is the change in entropy, and T is the temperature in Kelvin.
At equilibrium, ΔG will be equal to zero, so we can set up the equation:
0 = ΔH - TΔS
Rearranging the equation, we get:
TΔS = ΔH
Now we can substitute the given values into the equation and solve for T:
T = ΔH / ΔS
Now we can calculate the value of T:
T = 81.2 kJ / 128 J/K = 81,200 J / 128 J/K = 635 K
Now that we have the temperature, we can use it to calculate K using the equation:
K = e^(-ΔG/RT)
Where e is Euler's number approximately equal to 2.71828.
Since ΔG is zero at equilibrium, the equation simplifies to:
K = e^0 = 1
Therefore, the value of the equilibrium constant (K) for this reaction is 1.
None of the given options (a, b, c, d, e) match the calculated value of 1, so it seems there may be an error in the given answer choices.