Varies with temperature p636 fig 157 k value 10 5

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Unformatted text preview: nt. •varies with temperature p636: Fig. 15.7 K value 10-5 Reaction Hardly occurs 10-3 1 103 Reactants & products Co-exist in equilibrium 105 Goes to completion Questions involving Equilibrium Calculations K = 3.3×10-13 for AgBr(s) -16 K = 1.5 ×10 for AgI(s) Ag+ (aq) + Br - (aq) + - Ag (aq) + Cl (aq) (a) If [Ag+] = 5.7×10-7 M, what is [Br-] at equilibrium? K = [ Ag + c ][ Br − c ] K = [ Ag + c ][ Br − c ] = (5.7 ×10−7 M /1M ) ⋅ [ Br − /1M ] = 3.3 ×10−13 − −7 [ Br ] = 5.8 ×10 M (b) Is AgI(s) more soluble than AgBr(s)? Explain. No, it is less soluble …. K (AgI)is smaller! Question: Given that when K = 1 for this reaction N2(g) + 3H2(g) ↔ 2 NH3(g) H = + 92 kJ there are [N2] = [H2] = [NH3] = 1.0 mol/L, If the reaction vessel is suddenly decrease to ½ of its existing size, what is Q at that “instant”? 2 2 ([ NH 3 ] c ] K= K= 3 ([ N 2 ] c ) ⋅ ([ H 2 ] c ) (1mol / L /1mol / L) (1mol / L /1mol / L) ⋅ (1mol / L /1mol / L) 3 =1 Concentration = 1.0 mol ÷ 0.5 L = 2.0 M 2 Q= (2mol / L /1mol / L) (2mol / L /1mo...
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This document was uploaded on 02/26/2014.

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