Multiple Choice
For the reaction CO (g) + Cl2 (g) ⇌ COCl2 (g) with Kc = 255 at 1000 K, if the initial concentrations are [CO] = 0.1510 M and [Cl2] = 0.175 M, what is the equilibrium concentration of COCl2?
16. Chemical Equilibrium
Equilibrium Constant Calculations
Back16. Chemical Equilibrium
Equilibrium Constant Calculations
- Multiple Choice
The reaction: 2 NO(g) + Br2(g) ⇌ 2 NOBr(g), has a Kp of 2.5 x 102 at 35°C. Calculate the equilibrium concentration of NOBr, if equilibrium concentrations of NO and Br2 are 0.2 atm and 0.050 atm, respectively.
- Multiple Choice
For the reaction below, Kc = 1.5 at a constant temperature. A 3.2 L flask contains an equilibrium mixture of 3 compounds: 3.7 g of NH4HS, 70. g of NH3 and unknown amount of H2S. What is the mass (grams) of H2S produced at equilibrium?
NH4HS(s) ⇌ NH3(g) + H2S(g)
- Multiple ChoiceGiven the equilibrium CO(g) + H2O(g) ⇌ CO2(g) + H2(g) with an equilibrium constant (Keq) of 302 at 600K, what is the equilibrium constant for the reverse reaction CO2(g) + H2(g) ⇌ CO(g) + H2O(g) at the same temperature?
- Multiple ChoiceGiven the equilibrium expression 0.0611 = x^2 / ((1370 - x)(1710 - x)), what is the value of x at equilibrium?
- Multiple ChoiceGiven the equilibrium reaction 2CO(g) + O2(g) ⇌ 2CO2(g) with Kc = 2.8 × 10^2 at 298 K, and the partial pressures of CO and O2 are 5.168 × 10^-8 torr and 0.988 torr respectively, what is the partial pressure of CO2 in this mixture?
- Multiple ChoiceAt a certain temperature, Kc equals 1.4 × 10^2 for the reaction: 2 CO(g) + O2(g) ⇌ 2 CO2(g). If a 2.50-L flask contains 0.400 mol of CO2 and 0.100 mol of O2 at equilibrium, how many moles of CO are also present in the flask?
- Multiple ChoiceA solution initially contains [Ag+] of 3.2 × 10^-3 M and 0.125 M NH3. What is the concentration of Ag+ after the solution reaches equilibrium, given that the formation constant (Kf) of Ag(NH3)2+ is 1.7 × 10^7?
- Multiple ChoiceAn equilibrium mixture of CO, O2, and CO2 at a certain temperature contains 0.0010 M CO2 and 0.0020 M O2. At this temperature, Kc equals 1.4 × 10^2 for the reaction: 2 CO(g) + O2(g) ⇌ 2 CO2(g). What is the equilibrium concentration of CO?
- Multiple ChoiceAt a certain temperature, the equilibrium constant, Kc, equals 0.11 for the reaction: 2 ICl(g) ⇌ I2(g) + Cl2(g). What is the equilibrium concentration of ICl if 0.45 mol of I2 and 0.45 mol of Cl2 are initially mixed in a 2.0-L flask?
- Multiple ChoiceWhat is the equilibrium constant expression for a reaction at equilibrium?
- Multiple ChoiceCalculate the equilibrium constant (K) for the reaction: 2 N2O (g) + 3 O2 (g) ⇌ 2 N2O4 (g), using the following information: 1) 2 N2 (g) + O2 (g) ⇌ 2 N2O (g) K1 = 1.2 x 10^-35 2) N2O4 (g) ⇌ 2 NO2 (g) K2 = 4.6 x 10^-3 3) ½ N2 (g) + O2 (g) ⇌ NO2 (g) K3 = 4.1 x 10^-9
- Multiple ChoiceGiven the equilibrium reaction: H₂C₂O₄ ⇌ 2H⁺ + C₂O₄²⁻, calculate the equilibrium concentration of C₂O₄²⁻ in a 0.20 M solution of oxalic acid, assuming the acid dissociates completely. The equilibrium constant, Kₐ, for the first dissociation is 5.5 x 10⁻².
- Multiple ChoiceGiven the reaction Fe²⁺(aq) + Mn(s) ⇌ Fe(s) + Mn²⁺(aq), calculate the equilibrium constant (K) at 25°C if the concentrations at equilibrium are [Fe²⁺] = 0.010 M and [Mn²⁺] = 0.020 M. Express your answer to two significant figures.
- Multiple ChoiceConsider the following reaction: 2CH4(g) ⇌ C2H2(g) + 3H2(g). The reaction of CH4 is carried out at some temperature with an initial concentration of [CH4] = 0.089 M. At equilibrium, the concentration of H2 is 0.010 M. Find the equilibrium constant (Kc) for the reaction.