Which substance in each of the following pairs would have the greater entropy? E

Question

Which substance in each of the following pairs would have the greater entropy? Explain. (a) at 75degreeC and 1 atm: 1 mol H_2O(1) or 1 mol H_2O(g) (b) at 5degreeC and 1 atm: 50.0 g Fe(s) or 0.80 mol Fe(s) (c) 1 mol Br_2 (1, 1 atm, 8degreeC) or 1 mol Br_2 (s, 1 atm, -8degreeC) (d) 0.312 mol SO_2 (g, 0.110 atm, 32.5degreeC) or 0.284 mol O_2(g, 15.0 atm, 22.3degreeC) 7. For each of the following reactions, indicate whether DeltaS for the reaction should be positive or negative. If it is not possible to determine the sign of DeltaS from the information given, indicate why. (a) CaO(s) + H_2O(1) rightarrow Ca(OH)2(s) (b) 2 HgO(s) rightarrow 2Hg(1) +O_2(g) (c) 2 NaCl(1) rightarrow 2 Na(1) + Cl_2(g)

Explanation / Answer

6) (a) Greater the randomness or disorder, more is the entropy value.Thus, 1 mole of H2O(g) will have more entropy.
(b) molar mass of Fe = 56 g/mole

THus, mass of 0.8 mole of Fe = moles*molar mass = 44.8 g

Thus, 50 g of Fe(s) will have more entropy value.

c) Gretare the temperature, more is the K.E and more is the disorder.Thus, 1 mole of Br2 at 80C will have greatre entropy value

d) 0.312 moles of SO2 will have greater entropy value

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