Identify the reaction/process in which the entropy increases.
State $$1 \rightleftharpoons$$ State $$2 \rightleftharpoons$$ State 3 $$\left(\begin{array}{l}T=300 \mathrm{~K} \\ p=15 \mathrm{bar} \\ 1 \mathrm{~mol}\end{array}\right)\left(\begin{array}{l}T=300 \mathrm{~K} \\ p=10 \mathrm{bar} \\ 1 \mathrm{~mol}\end{array}\right)\left(\begin{array}{l}T=300 \mathrm{~K} \\ p=5 \mathrm{bar} \\ 1 \mathrm{~mol}\end{array}\right)$$
Above shows a cyclic process. Calculate the total work done during one complete cycle. [Assume a single step to reach the next state].
The formation of ammonia from its constituent elements is an exothermic reaction. The effect of increased temperature on the reaction equilibrium is
Equal volumes of 0.5 N acetic acid and 0.5 N sodium acetate are mixed. What is the pH of resultant solution? ($$\mathrm{p} K_a$$ of acetic acid $$=4.75$$)