Back to THERMODYNAMICS
NEET UG CHEMISTRY MCQ: THERMODYNAMICS
1
Hard
1 of 1
Understanding
+4 | -1
STATEMENT-1 : The standard free energy changes of all spontaneously occuring reactions are negative.
STATEMENT-2 : The standard free energies of the elements in their standard states at 1 bar and 298 K are taken as zero.
STATEMENT-2 : The standard free energies of the elements in their standard states at 1 bar and 298 K are taken as zero.
View answer and explanation
Correct option: B
If both the statements are TRUE but STATEMENT-2 is NOT the correct explanation of STATEMENT-1
Both statements are true, but the second statement does not explain the first. Spontaneous reactions have negative Gibbs free energy changes, and the standard free energies of elements in their standard states are defined as zero.
More Questions from THERMODYNAMICS
Practice All Chapter MCQs →
The internal energy of one mole of a gas is:
An ideal gas is allowed to expand both reversibly and irreversibly in an isolated system. If is the initial temperature and is the final temperature, which of the following statements is correct?
For which of the process, ∆S is negative?
The work done by a weightless piston in causing an expansion ∆V (at constant temperature), when the opposing pressure, P is variable, is given by:
Assertion :- At constant pressure of the change work done is negative.
Reason :- During phase transition work done is always negative. For the reaction, at . Hence, is
Reason :- During phase transition work done is always negative. For the reaction, at . Hence, is