Ncert Exercises & Solutions

Q.22. Calculate the entropy change in surroundings when 1.00 mol of $H_{2} O_{(l)}$ is formed under standard conditions. $∆_{f} H^{θ} = - 286 k J m o l^{- 1}$ .

NEETprep Answer:

The positive value of ∆rH indicates that heat is absorbed during the formation of NO(g).
This means that NO(g) has higher energy than the reactants (

N_{2} a n d O_{2}

). Hence, NO(g) is unstable.
The negative value of ∆rH indicates that heat is evolved during the formation of NO2(g) from
NO(g) and

O_{2}

(g). The product,

N O_{2 (g)}

is stabilized with minimum energy.
Hence, unstable NO(g) changes to unstable

N O_{2 (g)}

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