Determine the equilibrium constant for the following reaaction at 298K.
SO3(g)+J2O(g)->H2SO4(l); delta G = -90.5
dG = -RT*ln*K
Use 8.314 for R
dg=dG+rtlnk
To determine the equilibrium constant (K) for a reaction, we need to use the equation:
ΔG = -RT ln(K)
Where:
- ΔG is the standard Gibbs free energy change for the reaction
- R is the gas constant (8.314 J/(mol·K))
- T is the temperature in Kelvin (298K)
- K is the equilibrium constant we want to find
Given that the ΔG is -90.5, we can rearrange the equation to solve for K:
K = e^(-ΔG / (RT))
Plugging in the values:
K = e^(-(-90.5) / (8.314 * 298))
Now we can calculate the value of K using a scientific calculator or software.