Determine whether the entropy increases or decreases in the first process. In th

Question

Determine whether the entropy increases or decreases in the first process. In the first process, nitrogen gas is compressed from a volume of 2.0 L to 1.5 L at a constant temperature. When the gas is compressed, its positions to occupy (in the container) and freedom of motion. Based on the information in Step 2. we can predict that the entropy of the system Given a chemical or physical process, prided whether entropy Increases or decreases. The reaction below is performed in a bomb calorimeter (constant volume), with an accompanying release of heat. 2 H_2 (g) + O_2 (g) rightarrow 2 H_2 O (g) Delta H = -483.6 kJ Determine whether the entropy increases or decreases in the second process. The second process, occurring at constant volume, is given. 2 H_2 (g) + O_2 (g) - 2 H_2 O (g) The chemical equation shows that moles of reactants are converted to moles of the product. The reaction occurs at a constant volume, and its enthalpy change (Delta H =-463.6 kJ) indicates that it is. Since the reaction involves in the nuttier of molecules m the system, the molecules have permutations in space (microstates) available to them. We can therefore predict that the entropy of the system. more or fewer greater or less increases or decreases exothermic or endothermic more or less increases or decreases

Explanation / Answer

Ans. Consider a scenario- you came first in the auditorium with 100 chairs. You can change your position from time to time as you please. After some time, 90 more people enter the hall and occupies the chairs. So, now you change your position only to vacant chairs (= 10). So, after hall is filled, you have least options to change your position – your entropy (freedom to change position- a sort of) has decreased!

# Part A. Similarly, compression makes molecules closer in a small volume. As a result, the molecules are closely packed- so have fewer positions to occupy, and it decrease the entropy (degree of randomness).

            Thus, A= fewer        , B = less       , C= decrease

#B. Part B.

The chemical equation shows that D. 3 moles of reactants (2 mol H2 + 1 mol O2) are converted to E. 2 moles of the product (2 mol H2O).

F = exothermic. The -ve sign indicates that energy is being released during the formation of product.   

G = less (better as “decrease”). 3 moles reactants are converted to 2 mol product. Therefore, the total number of molecules in reaction mixture decrease as the reaction progresses.

H = decreases (or, better as "less")         ; I = Increased – decrease in number of molecules in a reaction vessel increases free space available per molecule- so, now molecules have greater degree of randomness or entropy.

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