1. The following reaction run at 700 K produces hydrogen for use as a fuel. COle + H2O@) 2 Hz@) + CO2@) Keg = 8.3 at 700 K At equilibrium, analysis shows 0.200 atm of CO, 0.230 atm of H20, and 0.950 atm of CO2. What is equilibrium pressure of hydrogen? [T/, 3]

Kc = 0.76 at a given temperature for the reaction: 2 HI (g) = H2 (g) + l2 (g) . Consider the condition [HI] = 0.36 M and [H2] = [12] = 0.60 M. Which of the following statements is correct? a) The quotient Q > Kc. b) The reaction will shift to right to establish equilibrium. O a) only O b) only Both a) and b) are correct. neither a) nor b) is correct.

At a certain temperature, the ?p for the decomposition of H2S is 0.770.   H2S(g)↽−−⇀H2(g) + S(g)   Initially, only H2S is present at a pressure of 0.268 bar in a closed container. What is the total pressure in the container at equilibrium? Ptotal=                                                     bar

Consider the reaction, 2AB2(g) = A2(g) + 2B2(g), Kc = 0.263 at 25°C. The reaction begins with an unknown concentration of AB2 in the reaction flask. At equilibrium, the concentration of AB2 is found to be 0.00545 M. a) Complete the ICEE table below, b) Write the equilibrium expression and equation for this reaction (pay close attention to coefficients!), c) Calculate the equilibrium concentration of both products, and d) Calculate the initial concentration of AB2. You should confirm that your equilibrium concentrations will give the correct equilibrium constant when plugged into the expression. ICEE table I C E 2 AB₂(g) A₂(g) + 2 B₂(g)

Consider the following system at equilibrium where AH = 268 kJ and Kc = 5.10 × 10-6, at 548 K. NH4Cl(s) NH3(g) + HCl(9) The production of NH3(g) is favored by (indicate true or false): decreasing the temperature: decreasing the pressure (by changing the volume): increasing the volume: adding NH4Cl: adding HCl:

q The equilibrium constant, Ke, for the following reaction is 1.80 x 104 at 298 K. [Review Topics] [References] Use the References to access important values if needed for NH4HS(9) NH3(g) + H₂S(9) Calculate the equilibrium concentration of H₂S when 0.322 moles of NH4HS(s) are introduced into a 1.00 L vessel at 298 K. [H₂S] = M Submit Answer Show Hint NOV 30 Le... The equilib tv Retry Entire Group 9 more group attempts remaining Email In M

Consider the following reaction where Kc PC15 (9) PC13 (g) + Cl₂ (9) A reaction mixture was found to contain 0.117 moles of PC15 (g), 0.0259 moles of PC13 (g), and 0.0368 moles of C1₂ (g), in a 1.00 liter container. Calculate c Qc² = = 0.0120 at 500 K. Is the reaction at equilibrium? If not, what direction must it run in order to reach equilibrium? O The reaction must run in the forward direction to reach equilibrium. O The reaction must run in the reverse direction to reach equilibrium. O The reaction is at equilibrium.

3. For the following reaction: 2HI +> Hz + 2 K. = 0.0025 at 800.0 K Assuming you start with 8.00 moles of H2, and 8.00 moles of I, in a 2.00 L vessel, what are the concentrations of the reactants and products at equilibrium? Calculate the percent reaction. E