HW4_2 - + 6 KOH(aq) ----> KClO 3 (aq) + 5 KCl(aq) + 5 H...

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Homework due 4/2 Indicate whether the entropy change for the following reactions would be positive or negative. Justify your choice. a) N 2 (g) + 3 H 2( g) ------------->2 NH 3 (g) Negative - there are 4 molecules of gas in the reactants and only 2 in the products, thus the randomness of the system (the entropy of the system) will decrease. b) CaCl 2 (s) + H 2 SO 4 (l) ----> CaSO 4 (s) + 2 HCl(g) Positive - the fact that the gas HCl is produced will cause the entropy of the products to be greater than the entropy of the reactants. c) 3 Cl 2 (g)
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Unformatted text preview: + 6 KOH(aq) ----> KClO 3 (aq) + 5 KCl(aq) + 5 H 2 O(l) Negative- the fact that a gas is present in the reactants and not in the products will cause the entropy of the reactants to be greater than the entropy of the products, hence the entropy change for the reaction will be negative. d) 2 AgNO 3 (aq) + BaCl 2 (aq) ------> 2 AgCl(s) + Ba(NO 3 ) 2 (aq) Negative- the formation of the solid product will decrease the entropy of the system, thus making the entropy change for the reaction negative....
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This note was uploaded on 04/03/2008 for the course CHEM 114 taught by Professor Martin during the Spring '08 term at Moravian.

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