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Consider each of the following reactions and decide whether the standard entropy change for the reaction...

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Chemistry

Consider each of the following reactions and decide whether thestandard entropy change for the reaction will be large &positive; or small; or large & negative. 1. large&negative2. large&positive 3.small

a) H2(g) + Cl2(g) = 2 HCl(g)

b) 2 Na(l) + H2(g) = 2 NaH(s)

c) 2 H2O(l) = 2 H2(g) +O2(g)

d) C(s) + H2O(g) = CO(g) + H2(g)

e) Cu(s) + 2 H2SO4(aq) =CuSO4(aq) + 2 H2O(l) + SO2(g)

f) BaSO4(s) + 2 H2O(g) =BaSO4.2H2O(s)

2. Identify the true statement(s) regarding the entropy ofchemical substances.

All pure substances have a positive entropy at roomtemperature.

The dissolution of an ionic salt in water usually leads to anincrease in entropy of the system (salt + water).

So(one mole O3(g)) > So(onemole O2(g)) at 25oC.

The entropy of ice at 0oC is lower than that of waterat 0oC.

When a metallic crystal is heated, its entropy increases due toincreasing atomic vibrations.

Answer & Explanation Solved by verified expert
4.3 Ratings (589 Votes)
The sign of S will be positive if there is an increase in temperature an increase in the volume in which the molecules move or an increase in the number of gas particles in the reaction The question states that the temperature is constant Thus we need    See Answer
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