Question

Indicate whether you would expect the entropy of a system to increase or decrease of the following: (See lesson - 10) (i) N2 (g) + 3H2 (g) тЖТ 2NH3 (ii) O2 (g) тЖТ 2O(g)

Answer 1

(i) Entropy decreases as there is less no. of moles of gas in the product side. So, less randomness in product side than that in the reactant side.

(ii) Here, Entropy is increasing as there are more no. of moles of gas in the product side so randomness increases.

Answer 2

$N_2(g)+3H_2(g)\rightarrow 2NH_3(g)$ : Entropy will decrease

$O_2(g)\rightarrow 2O(g)$ : Entropy will increase

Explanation:

Entropy is the measure of randomness or disorder of a system. If a system moves from  an ordered arrangement to a disordered arrangement, the entropy is said to decrease and vice versa.

For the reaction:

a) $N_2(g)+3H_2(g)\rightarrow 2NH_3(g)$

In this reaction 4 moles of gaseous reactants are converting to 2 moles of gaseous products. The randomness will decrease and hence entropy will also decrease. Thus $\Delta S$ is negative.

b) $O_2(g)\rightarrow 2O(g)$

In this reaction 1 gaseous molecule is getting converted to two gaseous  atoms thus the randomness will increase and hence entropy will also increase.Thus $\Delta S$ is positive.

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