H2 and Ci2 are mixed together, initially without any product, HCI. The system is monitored over time as it comes to equilibrium. What would the graph of the concentration of H2 look like over time? A B Time Time ('H] [H,)

Question is attached.

Iodine reacts with bromine to produce IBr (iodine monobromide). I2(g) + Br2(g)  →  2IBr(g) At 150°C, Kc is 120. If 0.050 mols of IBr are placed in a 1.00L container, what is the concentration of IBr at equilibrium? A. 120 mol C. 0.50 mol D. 0.043 mol E. 0.00386 mol

What will the concentration of PCl5 be when equilibrium is reestablished after addition of 1.31 g Cl2? PCl5(g) ⇆ PCl3(g) + Cl2(g) Original Equilibrium Mixture: 3.95 g PCl5 4.86 g PCl3 3.59 g Cl2 in a 1.00-L flask. [PCl5] = ? mol/L

Consider the reaction. NaC2O2H3(s) <--- H2O ------> NaC2O2H3(aq), which is at equilibrium in an open flask in the lab at room temperature. You add more water to the equilibrium mixture. When the system reestablishes equilibrium, what has changed?  a. the concentration of NaC2H3O2(aq) does not change b. heat is produced c. the concentration of NaC2H3O2(aq) decreases d. the concentration of the water increases

Decide whether each of the following statements is true or false.  If false, change the wording of the statement to make it true.   a) The magnitude of the equilibrium constant is always independent of temperature. b) When two chemical equations are added to give a net equation, the equilibrium constant for the net equation is the product of the equilibrium constants of the summed equations. c) The equilibrium constant for a reaction has the same value as K for the reverse reaction.  d) Only the concentration of CO2 appears in the equilibrium expression for the reaction: CaCO3 (s) ↔ CaO (s) + CO2 (g). e) For the reaction CaCO3 (s) ↔ CaO (s) + CO2 (g), the value of K is numerically the same whether the amount of CO2 is expressed as molarity or as gas pressure.

Chapter 1 question 6: Ammonia has been studied as an alternative "clean" fuel for internal combustion engines, since its reaction with oxygen produces only nitrogen and water vapor, and in the liquid form it is easily transported. An industrial chemist studying this reaction fills a 50.0L tank with 4.6 mol of ammonia gas and 4.5 mol of oxygen gas, and when the mixture has come to equilibrium measures the amount of nitrogen gas to be 1.2 mol. Calculate the concentration equilibrium constant for the combustion of ammonia at the final temperature of the mixture. Round your answer to 2 significant digits.

When considering the reaction at equilibrium which direction will the reaction shift (left, right, no effect) to compensate for the following permutations? 1. Adding more HNO3. 2. Siphoning off the N2. 3. Decreasing the temperature of the system. 4. Increasing the pressure of the system.

Jon and Sally have set up an equilibrium system on their lab bench. If they increase the temperature, which will be affected? I. equilibrium concentrations II. the value of the equilibrium constant III. neither A) I only B) II only C) Ш only D) I and II

6. Consider the reaction: N2 (g) + 3 H2 (g) = 2 NH3 (g) Complete the table below, assuming all concentrations are equilibrium concentrations in. molarity. TK IN2] [H2] ENH3] Kc 500 0.115 0.105 0.439 575 0.110 0.128 9.6