ThermodynamicsHard
Question
A system undergoes a process in which the entropy change is +5.51 JK–1. During the process, 1.50 kJ of heat is added to the system at 300 K. The correct information regarding the process is
Options
A.the process thermodynamically reversible.
B.the process is thermodynamically irreversible.
C.the process may or may not be thermodynamically reversible.
D.the process must be isobaric.
Solution
$\Delta S_{\text{Surr}} = - \frac{1.5 \times 10^{3}}{300} = - 5\text{ J/K}$
$\text{Now, }\Delta S_{\text{unit}} = \Delta S_{sys} + \Delta S_{\text{surr}} = 5.51 + ( - 5) = + 0.51\text{ J/K}$
Hence, the process is irreversible.
Create a free account to view solution
View Solution FreeMore Thermodynamics Questions
A container of volume 1 m3 is divided into two equal parts by a partition. One part has an ideal diatomic gas at 300 K a...Which of the following is correct option for free expansion of an ideal gas under adiabatic condition ?...Standard entropy of X2, Y2 and XY2 are 60, 40 and 50 JK-1mol-1, respectively. For the reaction,, ᐃH = - 30 kJ, to ...For the reaction, , graph is plotted as shown below. Identify correct statements.A. Standard free energy change for the ...The dissolution of NH4Cl in water is endothermic even through NH4Cl dissolves in water spontaneously. Which one of the f...