What is the value of delta G at melting point of ice?
To determine the value of ΔG (delta G) at the melting point of ice, we need to use the equation ΔG = ΔH - TΔS, where ΔH is the enthalpy change, ΔS is the entropy change, and T is the temperature in Kelvin.
First, let's find the values for ΔH and ΔS of the phase transition from solid to liquid (melting) for ice:
- The enthalpy change, ΔH, is the heat energy required to convert one mole of a substance from solid to liquid at constant temperature and pressure. For the melting of ice, the value of ΔH is approximately 6.01 kilojoules per mole (kJ/mol).
- The entropy change, ΔS, is a measure of the disorder or randomness of a system. For the melting of ice, the value of ΔS is approximately 22.0 J/(mol·K).
Now, we need to know the melting point of ice. The melting point of ice is 0 degrees Celsius or 273.15 Kelvin.
Plugging these values into the equation:
ΔG = ΔH - TΔS
ΔG = (6.01 kJ/mol) - (273.15 K) * (22.0 J/(mol·K))
To convert the units, we need to multiply ΔS by 1000 to ensure it is in kilojoules (kJ):
ΔG = (6.01 kJ/mol) - (273.15 K) * (22.0 J/(mol·K)) * (1 kJ/1000 J)
Calculating this equation will give you the value of ΔG at the melting point of ice.