The standard free energy change for a chemical reaction is -18.3kJ/mole. What is the equilibrium constant for the reaction at 87 degrees Celsius? (R=8.314J/K*mol)
Delta G = -Rtlnk
-18,300/8.314/360 = -6.114
It looks like you solved for ln K
They asked for K.
I assume your -18,300/8.314/360 means
-18,300/(8.314*360)
Never write fractions as a/b/c
To find the equilibrium constant (K) for the reaction, we can use the equation:
ΔG = -RTlnK
Where:
ΔG is the standard free energy change for the reaction,
R is the gas constant (8.314 J/K*mol),
T is the temperature in Kelvin, and
K is the equilibrium constant we want to calculate.
Given that ΔG is -18.3 kJ/mol and T is 87 degrees Celsius, we need to convert the temperature to Kelvin by adding 273.15.
T = 87 + 273.15 = 360.15 K
Substituting the values into the equation, we have:
-18,300 J/mol = (-8.314 J/K*mol)(360.15 K) ln K
Dividing both sides by -8.314*360.15:
-18,300/8.314/360.15 = ln K
Calculating this will give us the natural logarithm of K. Therefore, we need to exponentiate both sides of the equation to find K. The exponential form of ln K is e^(ln K) = K. So, we can calculate K by raising e (approximately equal to 2.718) to the power of the left side of the equation:
K = e^(-18,300/8.314/360.15)
Evaluating this expression will give you the equilibrium constant (K) for the reaction at 87 degrees Celsius.