CO(g) + H₂O(g) = H₂(g) + CO₂(g) K= 7.3 @ 823 K A closed 5.0 L container initially holds 3.0 moles CO and 6.0 moles H₂0. Calculate the concentrations of each material at equilibrium. What is the equilibrium concentration of H₂O? [H₂O] = [?] M

A gaseous mixture contains 0.27 mol CO, 0.12 mol H2, and 0.022 mol H,O, plus an unknown amount of CH4, in each liter. This mixture is at equilibrium at a certain temperature. CO(9) + 3H, (9) = CH4 (9) + H,O(9) What is the concentration of CH4 in this mixture? The equilibrium constant K, equals 3.99.

3. Nitrogen gas and oxygen gas can combine to produce nitrogen monoxide. At 1500 K the equilibrium constant, Ke, is 1.0 x 10 . Suppose a sample of air has [N2] = 0.80 M and [O2] = 0.20 M before any reaction occurs. Calculate the equilibrium concentrations of product and reactants at equilibrium at this temperature.

The equilibrium constant K = 53.09 for H2(g) +12(g) 2 HI(g) has been determined at a certain temperature. If 1.00 mol each of H2 and 12 is placed in a 0.500-L flask at that temperature, what are the concentrations of H2, 12, and HI when equilibrium has been achieved? [H₂]= M [12]= M [H0] => M

At a certain temperature, this reaction establishes an equilibrium with the given equilibrium constant, Kç. 3 A(g) + 2 B(g) = 4 C(g) K = 1.33 x 102' If, at this temperature, 1.70 mol of A and 4.00 mol of B are placed in a 1.00 L container, what are the concentrations of A, B, and C at equilibrium? [A] = M [B] = M [C] = M

1. Consider the following reaction at 500 K: 2 NO (g) + O2 (g) 2 2 NO2 (g); Kc = 6.9 x 105 This reaction is allowed to reach equilibrium, and then analyzed and found to contain the following concentrations: [O2] = 1.0 x 10-3 M [NO2] = 5.0 x 10-2 M. Determine the equilibrium concentration of NO (g).

A chemist is studying the following equilibirum, which has the given equilibrium constant at a certain temperature: N2(g) + 2H2O(g) 2 NO(g) + 2 H2(g) K=2.x 10 -10 He fills a reaction vessel at this temperature with 6.0 atm of nitrogen gas and 11. atm of water vapor. Use this data to answer the questions in the table below. Can you predict the equilibrium pressure of H2, using only the tools available to you within ALEKS? ○ yes x10 O no If you said yes, then enter the equilibrium pressure of H₂ at right. Round your answer to 1 significant digit. atm 5

When 0.16 mol of O2 gas and excess graphite were placed in a 2.00-L container and come to equilibrium, the concentration of CO gas was 0.088 0.024 M. What is the equilibrium constant, Kc, for this reaction at this temperature? Please report 4 decimal places, without units. C(s) + O2(g) ⟷ 2CO(g)

At a certain temperature, the equilibrium constant, K., is 0.00572 for the reaction Cl,(g) = 2 Cl(g) A. If 2.77 g Cl, is placed in a 2.50 L flask at this temperature, what are the equilibrium concentrations of Cl, and Cl? [CI,] = M [CI] = M B. Following the establishment of equilibrium in part A, the volume of the flask is suddenly increased to 5.00 L while the temperature is held constant. What are the new equilibrium concentrations of Cl, and Cl? [Cl,] = M [CI] = M C. Following the establishment of equilibrium in part A, the volume of the flask is instead suddenly decreased to 1.0 L while the temperature is held constant. What are the new equilibrium concentrations of Cl, and CI? [Cl,] = M [CI] = M

CO2(g) + H2(g) « H2O(g) + CO(g) When H2(g) is mixed with CO2(g) at 2,000 K, equilibrium is achieved according to the equation above. In one experiment, the following equilibrium concentrations were measured.                                      [H2]  = 0.20 mol/L                                   [CO2]  = 0.30 mol/L                      [H2O] = [CO]  = 0.55 mol/L (a)   What is the mole fraction of CO(g) in the equilibrium mixture? (b)   Using the equilibrium concentrations given above, calculate the value of Kc, the equilibrium constant for the reaction. (c)   Determine Kp in terms of Kc for this system. (d)   When the system is cooled from 2,000 K to a lower temperature, 30.0 percent of the CO(g) is converted back to CO2(g). Calculate the value of Kc at this lower temperature. (e)   In a different experiment, 0.50 mole of H2(g) is mixed with 0.50 mole of CO2(g) in a 3.0-liter reaction vessel at 2,000 K. Calculate the equilibrium concentration, in moles per liter, of CO(g) at this…