A tiny sample of an aqueous solution of two substances R and P is sketched below, as if it was under an imaginary microscope so powerful that individual molecules could be seen. (The water molecules are not shown.) G00 R P 00 R and P can interconvert. That is, R can turn into P, and P can turn back into R: R(ag) P(ag) K= 3 The equilibrium constant K for this equilibrium is 3. Predict the number of R and P molecules in this sample when the interconversion reaches equilibrium. number of R molecules: number of P molecules:

Consider the following equilibria at a given temperature: ½Nalg) + J½O>(g) = NO(g) K= 6.45 x 10°, NO (g) + 1½Brz(g) = NOB((g) K= 1.40 Determine the value of the equilibrium constant for the following reaction at the same temperature: %N(g) + ½Ozlg) + ½Br2(g) = NOBr(g) OA 583 x 107 O B.3.36 x 10-18 OC4.17x 107 OD.6.45 x 10 OE 9.03 x 10

A student ran the following reaction in the laboratory at 591 K:COCl2(g) CO(g) + Cl2(g)When she introduced COCl2(g) at a pressure of 0.380 atm into a 1.00 L evacuated container, she found the equilibrium partial pressure of Cl2(g) to be 0.247 atm.Calculate the equilibrium constant, Kp, she obtained for this reaction.

[5] The following equilibrium constants were determined at 1123 K C(s) + CO(g) = 2CO(g) K = 1.3x 10¹4 -3 CO(g) + Cl₂(g) = COCI(g) K = 6.0x 10-³ Determine the equilibrium constant for the reaction C(s) + CO(g) + 3Cl2(g) = 2COCl2(g) at 1123K [6] For each of the following reactions convert between Kp and Kc a) Determine Kp at 1173K for the reaction CS2(g) + 4H₂(g) = CH4(g) + 2H2S(g) At this temperature Kc = 27.8. b) Determine Kc at 1100K for the reaction 2SO2(g) + O2(g) = 2SO3(g). At this temperature Kp = 0.25

Write equilibrium-constant expressions K, for each of the following reactions. PC|3(g) + 3NH3(g) D P(NH2)3g) + 3HC((g) 4NH3(g) + 502E)D 4NO(g) + 6H20(g) NazCO3(s) + SO23) + ½ O2(g) D Naz504(s) + CO2(g)