Consider the reaction A(g) + B(g)  C(g) + D(g). You have the gases A, B, C, and D at equilibrium. Upon adding gas A, the value of K: increases, because by adding A more products are made, increasing the product to reactant ratio decreases, because A is a reactant so the product to reactant ratio decreases does not change, because A does not figure into the product to reactant ratio does not change, as long as the temperature is constant depends on whether the reaction is endothermic or exothermic

Solid NH4HS decomposes by the following endothermic reaction:   NH4HS (s)       NH3 (g)     +     H2S (g) If the system was at equilibrium, what effect would each of the following have on the system.  For your answer, indicate whether the reaction shifts to the left, shifts to the right, or no change to reestablish equilibrium. a.  The concentration of NH3 is increased. b.  Additional NH4HS is added to the system. c.  The volume of the container the reaction is placed in increases. d.  The container that contains the reaction is cooled in an ice bath.

There are two parts to this question. Each part is attached in separate pictures.

Iron(III) oxide and hydrogen react to form iron and water, like this: Fe,O3(s)+3 H2(9)→2 Fe(s)+3 H,O(g) At a certain temperature, a chemist finds that a 4.5 L reaction vessel containing a mixture of iron(III) oxide, hydrogen, iron, and water at equilibrium has the following composition: compound amount Fe,O3 3.54 g H2 3.20 g Fe 4.49 g H,O 1.06 g Calculate the value of the equilibrium constant K¸ for this reaction. Round your answer to 2 significant digits.

The following reaction is investigated (assume an ideal gas mixture): 2N20(g) + N2H4(g) 3N2(g) + 2H2O(g) Initially there are 0.100 mol of N20 and 0.25 mol of N2H4, in a 10.0-L container. If there are 0.059 mol of N20 at equilibrium, how many moles of N2 are present at equilibrium? O 4.1 x 10^-2 1.2 x 10^-1 6.2 x 10A-2 O 2.1 x 10^-2 O none of these

The reaction below was allowed to react at 375 degrees Celcius until it formed an equilibrium. At equilibrium, the 16.2 L container was found to contain 1.9 mol SiF4, 1.1 mol H2O, 3.5 mol SiO2, and 2.9 mol HF. What is the Kc of the reaction at this temperature?  SiF4 (g) + 2H2O (g) <--> SiO2 (s) + 4HF(g)

The reaction 2A(s) + B(g) = 2C(s) represents a(n). A homogeneous equilibrium heterogeneous equilibrium c) instantaneous equilibrium D reaction that will not come to an equilibrium

7:42 Question 45 of 50 Submit The reaction of NO(g) + Cl₂(g) = NOCI(g) + Cl(g) is found to have an equilibrium constant of 1.1x10³ at a particular temperature. What does this mean? A) At equilibrium, there is a much higher concentration of reactants than products. B) At equilibrium, there is a much higher concentration of products than reactants. C) At equilibrium, there is an equal concentration of reactants and products. D) At equilibrium, the relative concentrations of reactants and products depends on the initial concentrations. Tap here or pull up for additional resources

7. Consider the following equilibrium: 2NOCI(g) = 2NO(g) + Cl2(g) K = 1.56 x 10-5 If 2.00 moles of pure nitrogen monoxide and 3.00 moles of pure chlorine gas are placed in a 2.00-L container, calculate the concentration of Cl2(g) once the reaction has reached equilibrium.

= KINETICS AND EQUILIBRIUM Setting up a reaction table Suppose a 500. mL flask is filled with 1.7 mol of N₂ and 0.10 mol of NH3. This reaction becomes possible: N₂(g) + 3H₂(g)2NH, (g) Complete the table below, so that it lists the initial molarity of each compound, the change in molarity of each compound due to the reaction, and the equilibrium molarity of each compound after the reaction has come to equilibrium. Use x to stand for the unknown change in the molarity of N₂. You can leave out the M symbol for molarity. initial change equilibrium N₂ 0 0 H₂ 0 0 0 NH3 0 0 00 1/5 X