The deltaS for a reaction is 3.0 J/(mol*K) at 25 degrees C. Caluculate the deltaG for the reaction when DeltaH = -394 kL and determine whether it will occur spontaneously at this temperature
delta G = delta H -T*deltaS
You must mean -394 kJ and not kL for DH.
What's the problem is just plugging in and getting the answer? The USUAL problem with students is they forget DH is in kJ and DS is in J.
So you want -394 kJ -(298.15)*.003 = ?? kJ.
If the sign is negative, the reaction is spontaneous. If +, the reaction is not spontaneous.
so would it be -2.0764 or do i need to move the decimal?
I don't know how you obtained -2.0764.
-394-(298.15*-0.003) = -394-0.894 = ??.
I changed 3 J/mol*K to kJ/mol*K.
To calculate the deltaG for a reaction, you can use the equation:
deltaG = deltaH - T * deltaS
where deltaG is the change in Gibbs free energy, deltaH is the change in enthalpy, T is the temperature in Kelvin, and deltaS is the change in entropy.
In the given question, the deltaH is given as -394 kJ/mol (note that it should be converted to J/mol). DeltaS is given as 3.0 J/(mol*K), and the temperature is 25 degrees Celsius. To perform calculations, we need to convert the temperature from Celsius to Kelvin:
T = 25 + 273.15 = 298.15 K.
Now, we can plug the values into the equation:
deltaG = (-394 * 10^3 J/mol) - (298.15 K * 3.0 J/(mol*K))
To obtain the answer, we need to perform the multiplication and subtraction:
deltaG = -394,000 J/mol - 894.45 J/mol
= -394,894.45 J/mol
Therefore, the value of deltaG for the reaction at 25 degrees Celsius is -394,894.45 J/mol.
To determine whether the reaction will occur spontaneously at this temperature, we can use the sign of deltaG. If deltaG is negative, the reaction is spontaneous, and if it is positive, the reaction is non-spontaneous.
In this case, since deltaG is negative, the reaction will occur spontaneously at 25 degrees Celsius.