Some COCI₂ is allowed to dissociate into CO and Cl₂ at 873 K. At equilibrium, [COCI₂] = 0.244 M, and [CO] = [Cl₂] = 0.130 M. Additional COCI₂ is added so that [COCI₂] new = 0.404 M and the system is allowed to once again reach equilibrium. CoCl₂(g)=CO(g) + Cl₂(g) K = 6.98×10-2 at 873 K (a) In which direction will the reaction proceed to reach equilibrium? (b) What are the new concentrations of reactants and products after the system reaches equilibrium? [COCI₂] = [CO] [Cl₂] = = M M M 4

The equilibrium constant, K, for the following reaction is 10.5 at 350 K. 2CH,Cl2(g) ? CH,(g) + CCl4(g) An equilibrium mixture of the three gases in a 1.00 L flask at 350 K contains 5.43x10-2 M CH,Cl,, 0.176 M CH, and 0.176 M CCL. What will be the concentrations of the three gases once equilibrium has been reestablished, if 0.124 mol of CH,(g) is added to the flask? [CH,Cl,] = M [CH4) M [CCL] M

An equilibrium mixture of PC1, (g), PC1, (g), and Cl₂ (g) has partial pressures of 217.0 Torr, 13.2 Torr, and 13.2 Torr, respectively. A quantity of Cl₂ (g) is injected into the mixture, and the total pressure jumps to 263.0 Torr at the moment of mixing. The system then re-equilibrates. The chemical equation for this reaction is PC1₂(g) + Cl₂(g) = PCl, (g) Calculate the new partial pressures, P, after equilibrium is reestablished. PPCL, Pch PPCL, = = = Torr Torr Torr

The equilibrium constant, Kc, for the following reaction is 57.6 at 277 K. 2CH₂Cl₂ (g) CH4 (9) + CCl4 (9) When a sufficiently large sample of CH₂Cl₂ (g) is introduced into an evacuated vessel at 277 K, the equilibrium concentration of CC14 (g) is found to be 0.383 M. Calculate the concentration of CH₂Cl₂ in the equilibrium mixture. [CH₂Cl₂] = M

Consider the equilibrium system described by the chemical reaction below. If the partial pressures at equilibrium of NO, Cl2, and NOCI are 0.095 atm, 0.171 atm, and 0.28 atm, respectively, in a reaction vessel of 7.00 L at 500 K, what is the value of Kp for this reaction? 2 NO(g) + Cl2(g) = 2 NOCI(g)

Consider the following reaction at a certain temperature: 4 Fe(s) + 3 O2(g)→ 2 Fe203(s) An equilibrium mixture contains 1.2 mol Fe, 0.00090 mol O2, and 2.0 mol Fez03 all in a 2.0-L container. Calculate the value of K for this reaction. K =

Some NOBR is placed in a sealed flask and heated to 385 K. When equilibrium is reached, the flask is found to contain NOBR (9.30×103 M), NO (1.27x102 M), and Br2 (1.18×102 M). What is the value of the equilibrium constant for this reaction at 385 K? 2NOBR(g)=2NO(g) + Br2(g) K=

Consider the equilibrium between SbCl5, SbCl3 and Cl₂. SbCl5(g) SbCl3(g) + Cl₂(g) K = 2.46x10-² at 530 K The reaction is allowed to reach equilibrium in a 7.30-L flask. At equilibrium, [SbCl5] = 0.430 M, [SbCl3] = 0.103 M and [Cl₂] = 0.103 M. (a) The equilibrium mixture is transferred to a 14.6-L flask. In which direction will the reaction proceed to reach equilibrium? (b) Calculate the new equilibrium concentrations that result when the equilibrium mixture is transferred to a 14.6-L flask. [SbCl5] = [SbCl3] = [Cl₂] |||| ΣΣΣ

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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.