Which one of the following equilibrium reactions is not affected by a change in pressure? H2(g) + 12(g) = 2HI(g) PCI3(g) + Cl2(g) = PCI5(g) 2NO2(g) = N204(g) O N2(g) + 3H2(g) = 2NH3(g)

The Keg for the equilibrium below is 7.82 · 10-2 at 510.0 °C. 2Cl, (g) + 2H20 (g) =4HCI (g) + 02 (g) What is the value of Keg at this temperature for the following reaction? Cl2 (g) + H20 (g) = 2HCI (g) + 02 (g) O 0.280 O 0.0376 O 6.12 - 10-3 O 0.150 O 0.0782

The equilibrium system shown below was analyzed and the concentrations of H2(g), I2(g) and HI(g), were found, in mol/L, to be 4.2, 3.8, 1.6 respectively. The equilibrium constant must be? H2(g) + I2(g) <=====> 2HI(g) + 65 kJ

The synthesis of CaCO3 uses this chemical reaction. CaO(aq) + CO2(g) ——> CaCO3(s) + 180 kJ Identify three stresses that can be imposed on the equilibrium to maximize the amount of CaCO3 present. Be specific about what, if any, compounds are involved in those stresses.

Consider this system at equilibrium. A(aq) = B(aq) AH = -350 kJ/mol What can be said about Q and K immediately after an increase in temperature? Q > K because Q increased. = K because neither changed. Q > K because K decreased. Q < K because K increased. О<к because Q decreased. How will the system respond to a temperature increase? shift right shift left no change

At a certain temperature, Keq = 135.5 for the following equilibrium: SO2(g) + NO2(g) <===> NO(g) + SO3(g) Suppose a reaction vessel at this temperature contained these three gases at the following concentrations: [SO2] = 0.00250 M, [NO2] = 0.00350 M, [NO] = 0.0250 M, [SO3] = 0.0400 M.  a)Determine Qeq for the system. (b)Is the system at equilibrium? If it is not, indicate the direction toward which the system will move to reach equilibrium.

For the following reaction at a certain temperature, 1.57 mol H2 and 1.56 mol l2 are placed into a 2.05 L flask. At equilibrium, 2.70 mol of HI has been formed. Calculate Kc. H2(g) + 12(g) = 2 HI(g)

Phosphorous pentachloride decomposes according to the reaction PCl5(g)↽−−⇀PCl3(g)+Cl2(g)PCl5⁢(g)⁢↽−−⇀⁢PCl3⁢(g)+Cl2⁢(g) A 13.1 gsample of PCl5 is added to a sealed 1.25 L flask and the reaction is allowed to come to equilibrium at a constant temperature. At equilibrium, 48.4% of the PCl5 remains. What is the equilibrium constant, Kc , for the reaction?

A student ran the following reaction in the laboratory at 588 K: CO(g) + Cl₂(g) —COCI₂(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 1.74 atm and the initial partial pressure of Cl2 was 0.951 atm, she found that the equilibrium partial pressure of COCI₂ was 0.685 atm. Calculate the equilibrium constant, Kp, she obtained for this reaction. Кр =