For each of the following pairs, which has the greater entropy? Assume that a ex

Question

For each of the following pairs, which has the greater entropy? Assume that a explicitly mentioned are the same for each part of the pair. ll variables not (a) A mole of N2 at 0°C or (a) a mole of N2 at 100°C. (b) A mole of N t 1 bar or (b') a mole of N2 at 100 bar. (c) 1 g of gypsum (CasO4) and 1 L of H20 or (c') 1 g of gypsum in 1 L of H20 after reaction. Hg at 1 bar is -38.83 °C The clay weathering product of a granite or (d) 1 mole of Hg at 25 °C or (d) 1 mole of Hg at -40 °C. Note that the freezing point of e) A granite or (e) the clay that results from granite weathering. the river water with the solutes from the dissolved granite (assume no clay forms).

Explanation / Answer

(1)

1 mole of N2 at 1000C will have higher entropy, because at higher temperature the energy of molecules is higher which causes movements with high frequency so the randomness of the system also increases.

(2)

1 mole of N2 at 1 bar will have higher entropy, because at lower pressures the volume is greater and the molecules have larger space to move, while at higher pressures the volume decreases and the system becomes more compressed or 'organized'. Hence entropy decreases with increase in pressure.

(3)

When the reaction takes place, heat is released, so the system becomes more organized. Hence the entropy of CaSO4 and 1 L water is higher before the reaction.

(4)

1 mole of Hg at 250C has higher entropy, because at temperature of -400C, Hg is in solid form which is more organized and hence has lesser entropy.

Hope this helps !

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