Question

6) Distrubuting Equilibrium a) The equilibrium constant, K, for the following reaction is 10.5 at 350 K 2CH2Cl2(g)CH4(g + CCl4(g) An equilibrium mixture of the three gases in a 1.00 L flask at 350 K contains 5.32x10-2 M CH2C2, 0.172 M CH4 and 0.172 M CCI4. What will be the concentrations of the three gases once equilibrium has been reestablished, if 9.58x102 mol of CH4(g is added to the flask? CH2Cl2l [CH4 [CCI4] b) The equilibrium constant, K, for the following reaction is 2.69x102 at 622 K. COC2(g)CO(g +Cl2(g) An equilibrium mixture of the three gases in a 4.53 L container at 622 K contains 0.247 M COCI2. 8.14x10-2 M CO and 8.14x10 2 M Cl2 What will be the concentrations of the three gases once equilibrium has been reestablished, if the volume of the container is increased to 10.3 L? [COC12]- [CO] = Ch] c) The equilibrium constant, Kp, for the following reaction is 0.110 at 298 K NH4HS(s)NH3(g) + H2S(g) If ΔΗΡ for this reaction is 92.7 kJ, what is the value of Kp at 184 K? 7. LeChatelier's principle

Answer 1

equilibrium constant k =

[products concentration] / [ reactants concentration]

also [A] active mass = moles of A / total volume of solution in mole/ liter

[c]. Kp = 2.046

4- 0.172472 Ma Fui b addin o-/72-0.095B To Remain K Constant, on qddin Shitt- Left sids_and more product ie,「CH4/ tprpud for ctr M2 0:0 358 M2 Кр We kno) 8.31 4 104 218 B214 140x14 455.73 x/p 3 An (KP2) 2-342 + en (om) en (KA) 스이 35

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