A student ran the following reaction in the laboratory at 580. K: CO(g) + Cl2(g) COCl2(g) When she introduced CO(g) and Cl2(g) into a 1.00 L evacuated container, so that the initial partial pressure of CO was 2.59 atm and the initial partial pressure of Cl2 was 1.82 atm, she found that the equilibrium partial pressure of COCl2 was 1.44 atm. Calculate the equilibrium constant, Kp, she obtained for this reaction.

A student ran the following reaction in the laboratory at 322 K: 2CH2Cl2(g) CH4(g) + CCl4(g) When he introduced CH2Cl2(g) at a pressure of 0.357 atm into a 1.00 L evacuated container, he found the equilibrium partial pressure of CH2Cl2(g) to be 3.7310-2 atm. Calculate the equilibrium constant, Kp, he obtained for this reaction.

The equilibrium constant, Kc, for the following reaction is 10.5 at 350 K. 2CH2Cl2(g) CH4(g) + CCl4(g) Calculate the equilibrium concentrations of reactant and products when 0.244 moles of CH2Cl2 are introduced into a 1.00 L vessel at 350 K.

[CH2Cl2] =______M

[CH4] =_________M

[CCl4] =_________M

The equilibrium constant, Kc, for the following reaction is 5.1010-6 at 548 K. NH4Cl(s) NH3(g) + HCl(g) Calculate the equilibrium concentration of HCl when 0.395 moles of NH4Cl(s) are introduced into a 1.00 L vessel at 548 K.

[HCl] =________M

The equilibrium constant, Kp, for the following reaction is 10.5 at 350 K: 2CH2Cl2(g) CH4(g) + CCl4(g) Calculate the equilibrium partial pressures of all species when CH2Cl2(g) is introduced into an evacuated flask at a pressure of 0.701 atm at 350 K.

PCH2Cl2 =_____atm

PCH4 =______atm

PCCl4 =________atm

The equilibrium constant, Kp, for the following reaction is 1.0410-2 at 548 K: NH4Cl(s) NH3(g) + HCl(g) Calculate the equilibrium partial pressure of HCl when 0.395 moles of NH4Cl(s) is introduced into a 1.00 L vessel at 548 K.

P_HCl = ______atm