16. For the system CO + CO2(g) → CaCO(s) the equilibrium constant expression is a. [CO]...
Consider the system at equilibrium. 2CO(g)+O2(g)<--->2CO2(g)A. How will increasing the concentration of CO shift the equilibrium? B. How will increasing the concentration of Co, shift the equilibrium? C. How will adding a catalyst shift the equilibrium?
Which of the following expressions is the correct equilibrium-constant expression for the reaction below? 200(g) = CO2(g) + C(s) A. [CO][C]/[CO] B. K [CO] C. [CO] / [CO2) D. [CO]/[CO] E. 2[CO] /[CO][C] In which of the following reactions would increasing pressure at constant temperature not change the concentrations of reactants and products, based on Le Châtelier's principle? ООООО A. 2N, () + 0,02N,0 () B. N.O. (g) 2NO, (g) C. N2(g) + 3H2(g)2NH3 (9) D. N2 (9) + 202...
13. Given the following reaction: 2CO(g) + O2(g) & CO2(g) with K. = 4000. Ar equilibrium, the concentrations of O, and Co, are 0.10 M and 0.75 M, respectively. Calculate the concentration of CO at equilibrium.
The value of K. for the reaction C(s) + CO2(g) → 2CO(g) is 1.6. What is the equilibrium concentration of CO if the equilibrium concentration of CO2 is 0.50 M? A. 0.31 B. 0.80 c. 0.89 D. 0.75
At 850°C, the equilibrium constant K for the reaction 2CO(g) = C(s) + CO2(g) has a value of 0.0935. If the total pressure in the system at equilibrium is 1.000 atm, what is the partial pressure of carbon monoxide?
Write the equilibrium-constant expression for the equilibrium Cs) + CO2(g) = 200) The table that follows shows the relative mole percent of CO2 and Code) at a total pressure of 1 atm for several temperatures. Calculate the value of Ke at each temperature. Is the reaction exothermic or endothermic? Temperature (°C) 850 950 1050 1250 CO2 (mol %) 6.23 1.32 0.37 0.06 co (mol %) 93.77 98.68 99.63 99.94
29. Consider the following equilibrium CO2(g)+ H2()Co(g) + H20(g); Ke 1.6 at 1260 K Suppose 0.019 mol CO2 and 0.030 mol H2 are placed in a 3.00-L vessel at 1260 K. What is pressure of CO(g)? (R 0.0821 L atm/K mol) a. 4 atm b. 0.35 atm c. 1.6 atm d. 0.66 atm e. 1 atm
Consider the reaction C(s)+CO2(g)⇌2CO(g). When 1.66 mol of CO2 and an excess of solid carbon are heated in a 21.2 L container at 1100K, the equilibrium concentration of CO is 7.19×10−2 M . Part A What is the equilibrium concentration of CO2? Part B What is the value of the equilibrium constant Kc at 1100 K?
16. The only factor that changes the equilibrium constant of a chemical reaction is: A) pressure B) concentration C) volume D) temperature 17. Determine the effect of increased pressure on the system in the following equilibrium: C(graphite)+S2(g) CS2 (g) A) The equilibrium position SHIFT to the right B) The equilibrium position SHIFT to the left C) does not change the position of equilibrium D) The Le Chatelet principle does not apply to the system. 18. If the acetic acid dissociation...
1) The following reaction is an equilibrium reaction. CO2(g) + C(graphite) = 2 CO(g) A reactor initially contained only 0.20 atm CO2 gas in the presence of graphite at 25 °C and later the reaction reached an equilibrium. Answer the following questions. A) If Kis 2.25 at the given temperature above, calculate the equilibrium pressures of CO, and CO, respectively. [6 pts) B) Determine the Ke of the reaction above. [4 pts]