Consider this reaction at equilibrium: C(s) + H;0(g) = CO() + H2(8) Predict whether the reaction will shift left, shift right, or remain unchanged after each disturbance. a. Cis added to the reaction mixture. b. H2O is condensed and removed from the reaction mixture. c. CO is added to the reaction mixture. d. Hz is removed from the reaction mixture.

According to Le Chatelier's principle, does the equilibrium shift in the direction of products or reactants when N2 is added to the equilibrium mixture of each of the following reactions? a. 2NH3(g) ➞ 3H2(g) + N2(g) b. N2(g) +O2(g) ➞ 2NO(g) c. 2NO2(g) ➞ N2(g) +2O2(g)

At 900.0 K, the equilibrium constant (Kp) for the following reaction is 0.345. 2SO2 + O2 (g) →2 SO3 (g) At equilibrium, the partial pressure of SO₂ is 33.1 atm and that of O₂ is 15.0 atm. The partial pressure of SO3 is. O 172 O 6.93-10-4 38.0 75.4 O 4.57-10-3 atm.

4. The decomposition of PCI5 is shown below PCI5 2 PCI3 Find out if the reaction proceeds forward, backward or if the system is at equilibrium when a 1.00L container is filled with 0.400 mole PCI5, 0.500 mole PCI3 and 0.200 mol CI2. + CI2 Kc=0.029

For the reaction 2SO2(g) + O2g) 2SO3(2) If K. = 4.3 x 10° and the following concentrations are present: [SO2] = 0.010 M, [SO3] = 10 M, [O2] = 0.01 M. Which of the following statements is correct? A. The system is at equilibrium B. The system is not at equilibrium and is shifting from left to right C. The system is not at equilibrium and is shifting from right to left D. There is not enough information E. The system is at equilibrium and is shifting from left to right 3.

A 1.00 liter flask contained 0.24 mol NO2 at 700 K which decomposed according to the reaction 2 NO2(g) = 2NO(g) + O2(g). At equilibrium the amount of NO was measured to be 0.14 mol, what is the value of Kc? A. 9,6 x 103 B. 1.1 x 102 C. 9.8 x 102 D. 1,4 x 101 E. 5.7 x 103

Consider the reaction: A(g) = B(g) + C(g) Find the equilibrium concentrations of A, B, and C for each value of K. Assume that the initial concentration of A in each case is 1.0 M and that the reaction mixture initially contains no products. Make any appropriate simplifying assumptions. a. K. = 1.0 b. K. = 0.010 c. K. = 1.0 x 10-S

7.study the reaction. N2 (g)+3H2 (g)⇌NH3 (g)+92 kJ What can be done to shift the equilibrium position of this reaction toward the right? a.increase the concentration of the NH3 gas b.compress the reaction vessel c.introduce a catalyst d.increase the temperature