2 A → B + C has a Kc of 0.2. The reaction commences with initial concentrations C subscript(A) = 0.2 M, C subscript(B) = 0.2 M, and C subscript(C) = 0.2 M. In what direction does the reaction occur?  The reaction shifts to the right to reach equilibrium.  The reaction is already at equilibrium.  Cannot be determined without knowing the temperature.  The reaction shifts to the left to

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The equilibrium constant is 0.0900 at 25 °C for the reaction H2O (g) + Cl2O (g) ↔ 2HOCl (g) The reaction is taking place under the following conditions, a 1.0 L flask contains 1.0 mole of HOCl, 0.10 mole of Cl2O, and 0.10 mole of H2O.  Is this reaction at equilibrium?  If it is not, which direction will the system shift?

For the equilibrium, 2NO(g)+2H2(g)→N2(g)+2H2O(g), what will happen if it were in a rigid vessel and argon gas (Ar) were added to the system? Assume temperature remains constant. a. there will be no change in the equilibrium b. the equilibrium will shift toward reactants c. the equilibrium will be pushed forward d. there will be a change in the value of the equilibrium constant

The addition of CO to the equilibrium system given below will... CH4G) + H20(g) = CO(g)+3H2(g) have no effect A O cause the reaction to shift to right .BO cause the reaction to shift to left .CO increase the rate of the forward reaction .D

4. For the reaction CH4(g) + 2 H2S(g) = CS2(g) + 4 H₂(g) Kc = 3.59 at 900 °C. For each of the following measured concentrations determine whether the reaction is at equilibrium. If not, in which direction will the reaction proceed to get to equilibrium? [CH] [H₂S] [CS₂] [H2] Expt 1 Expt 2 Expt 3 1.15 1.07 1.10 1.20 1.20 1.49 1.51 0.90 1.10 1.08 1.78 1.68

Consider the following reversible reaction equation: 2502(g) + Oz(g) → 2503(g) Ka = 1.2 x 103 Complete the following sentences (a-e) by selecting the best choice from the dropdown menus. a) This is an example of a v equilibrium. b) At equilibrium, this system will contain mostly c) If more SO2 is added to this system at equilibrium, the reaction will shift towards the d) If oxygen gas is removed from this system at equilibrium, the reaction will shift towards the e) If the volume of this system at equilibrium is increased, the reaction will shift towards the

A sample of H,S(g) at 0.495 atm is placed in a container and the following reaction reaches equilibrium. What is the total pressure of all gases in the container? 2H2S(g) = 2H2(g) + S2(g) K, = 3.85 x 10-7 0.497 atm 0.215 atm 0.793 atm 0.624 atm 0.387 atm O O O

14.  The following reaction is allowed to come to equilibrium and then the volume is increased.  Predict the effect of the indicated volume change once equilibrium is restored.                         H2O(g)            +          CO2(g)               double arrow              H2CO3(g)     The reaction will shift right.     The reaction will shift left.     There will be no effect.     Effect can not be determined from information provided.

Bromine is one of the few elements that is a liquid at room temperature. It vaporizes easily and has a beautiful red color in both the liquid and gaseous states.Bromine reacts readily with hydrogen gas to make hydrogen bromide.One way to represent this equilibrium is:2 HBr(g)H2(g) + Br2(g)   We could also write this reaction three other ways, listed below. The equilibrium constants for all of the reactions are related. Write the equilibrium constant for each new reaction in terms of K, the equilibrium constant for the reaction above. 1) HBr(g)   1/2 H2(g) + 1/2 Br2(g)     K1 =   2) 1/2 H2(g) + 1/2 Br2(g)   HBr(g)   K2 =   3) H2(g) + Br2(g)   2HBr(g)   K3 =   Drag and drop your selection from the following list to complete the answer: K1/2(1/K)1/21/K