The G value for formation of gaseous water at 298 K and 1 atm is -278 kJ/mol. What is the nature of the spontaneity of formation of gaseous water at these conditions?
A. The reaction is sometimes spontaneous.
B. The reaction is spontaneous.
C. The reaction may or may not be spontaneous.
D. The reaction is never spontaneous.
A negative value for dG means it is spontaneous.
To determine the nature of the spontaneity of the formation of gaseous water at these conditions, we need to consider the sign of the Gibbs Free Energy (ΔG).
The Gibbs Free Energy (ΔG) can be calculated using the equation:
ΔG = ΔH - TΔS
Where:
ΔH is the change in enthalpy (heat) of the system,
T is the temperature in Kelvin,
ΔS is the change in entropy (disorder) of the system.
Given that the value of ΔG for the formation of gaseous water is -278 kJ/mol, which is negative, we can deduce that the reaction is spontaneous.
In spontaneous reactions, ΔG is negative, indicating that the reaction can occur without the need for an external driving force. This means that the formation of gaseous water at 298 K and 1 atm is a spontaneous process.
Therefore, the correct answer is B. The reaction is spontaneous.