What is the gibbs free energy for the reaction a)temperature b)800 degrees celsius c)comment on whether the reactions are spontaneous or not
(CHEMICAL REACTION) deltaH = -100kJ
delta S= -200 J/K
To calculate the Gibbs free energy (ΔG) of a chemical reaction, you can use the equation:
ΔG = ΔH - TΔS
Where:
ΔG is the Gibbs free energy
ΔH is the enthalpy change of the reaction
T is the temperature in Kelvin
ΔS is the entropy change of the reaction
In this case, you have the following values:
ΔH = -100 kJ
ΔS = -200 J/K
To calculate the Gibbs free energy at different temperatures, you will need to convert the temperature from degrees Celsius to Kelvin. The conversion is done by adding 273.15 to the Celsius temperature.
a) At an unspecified temperature:
To calculate ΔG at an unspecified temperature, you will need the specific value for temperature in Kelvin.
b) At 800 degrees Celsius:
To calculate ΔG at 800 degrees Celsius, you first need to convert the temperature to Kelvin.
T = 800 + 273.15 = 1073.15 K
Now, insert the values into the equation:
ΔG = ΔH - TΔS
ΔG = -100 kJ - (1073.15 K)(-200 J/K)
ΔG = -100 kJ + 214630 J
ΔG = 214530 J = 214.53 kJ
c) Determining spontaneity:
For a reaction to be spontaneous, the ΔG value should be negative (ΔG < 0). If ΔG is positive (ΔG > 0), the reaction is non-spontaneous.
- At an unspecified temperature, you cannot determine spontaneity without knowing the specific value of temperature.
- At 800 degrees Celsius, ΔG = 214.53 kJ, which is a positive value. Therefore, the reaction is non-spontaneous at 800 degrees Celsius.