notebook. the fume hoods, prepare asure 3 mL of water and level of 3 mL of solution ed. - bath to reduce bumping almly. brium test tube. rium system to go to the ent, add it dropwise until Loose only from the 1 M ter adding 10 drops, try rium system back to its dd it dropwise until the se only from the 1 M nt does not work, try ution into a test tube. = until you observe a esolution in a boiling agitate the test tube r2 min and then place als from time to time. -m the ice bath at the own "snow globe". d NH4Cl to cover the the sides of the test more NH4Cl. FeCl3 and 1 mL of 0.1 M KSCN in a 100-mL by combining 1 mL volumetric flask and filling the flask with DI H2O. Add 3 mL of this FeCl3-KSCN solution each to two test tubes. 2. To the first one, add 5 drops of 0.1 M FeCl3. 3. To the second one, add 5 drops of 0.1 M KSCN. After recording your observations, add 5 drops of 0.1 M AgNO3 to the same test tube. Mix the solution thoroughly and wait for 5 min. The white precipitate is AgSCN. Waste Disposal Liquids: hazardous waste Practice Problems . Problem 1: Consider the following reaction at equilibrium: N2(g) + 3H2(g) → 2NH3(g) AH-92 kJ/mol a) How is the pressure of ammonia affected if some nitrogen gas is added? b) How is the amount of hydrogen gas affected if the volume of the reaction vessel is doubled? How is K affected? c) How is the pressure of hydrogen gas affected if the temperature is raised? How is K affected? d) How are the rate of the reverse reaction and the pressure of hydrogen gas affected if a catalyst is added? Problem 2: Consider the following reaction at equilibrium: Zn(s) + 2HCl(aq) = ZnCl2(aq) + H2(g) a) How is [ZnCl2] affected if some HCl is added? b) Some hydrogen gas is removed. How does this affect the pH (pH = -log[H3O+])? c) Some NaOH is added. How does this affect the pH and the pressure of hydrogen gas? d) Some solid zinc is added. How does this affect [HC1]? Answers: 1a) increase, b) increase, no change, c) increase, decrease, d) increase, no change, 2a) increase, b) increase, c) increase, decrease, d) no change gas ever Lecree HCI loc A C 17 77

Write the equilibrium-constant expression for the reaction A(s) + 3 B(1) = 2C(aq) + D(aq) in terms of [A], [B], [C] , and [D] , as needed. Note that Ke, which is sometimes symbolized as Keg, denotes that the equilibrium constant is expressed using molar concentrations. For this question, K. means the same thing as Keq. K. =

4. Given the following system: 2CO, (g) 21CO (g) + 0, if the Keq = 6.40 x 10° @ 2000°C and initially 0.250 mol of CO; (g) is placed in a 1000mL reaction vessel, what are the equilibrium concentrations of all the entities? Confirm your answer by finding Q, the reaction quotient.

A monoprotic weak acid, HAHA, dissociates in water according to the reaction   HA(aq)↽−−⇀H+(aq)+A−(aq)HA(aq)↽−−⇀H+(aq)+A−(aq)   The equilibrium concentrations of the reactants and products are [HA]=0.220 M[HA]=0.220 M, [H+]=3.00×10−4 M[H+]=3.00×10−4 M, and [A−]=3.00×10−4 M[A−]=3.00×10−4 M. Calculate the value of p?ap�a for the acid HAHA.

You have two 250 mL beakers placed side by side under a bell jar, each filled with 100. mL of water, one containing 0.100 moles of NaCl, and the other containing 0.100 moles of CaCl2. After some time, equilibrium is established between the two beakers. What are the final volumes in the two beakers? (Assume ideal behavior, and that the sum of the two volumes remains 200. mL.)

Write the expressions for K, for the following reactions. In each case indicate whether the reaction is homoge- neous or heterogeneous. (a) 203(g) = 302(8) (b) Ti(s) + 2 Cl2(8) = TIC14(I) (c) 2 C,H,(8) + 2H,0(g) = 2 C,H¿(8) + O2(8)| (d) C(s) + 2 H2(8) = CH4(8) (e) 4 HCI(aq) + Oz(8) = 2 H20(1) + 2 Cl2(8) (f) 2 C3H18(1) + 25 O2(g) = 16 CO2(8) + 18 H20(g) (g) 2 C3H18(1) + 25 O2(8) 16 CO2(8) + 18 H20(I)

The equilibrium constant for the reaction: CO2(g) 2 CO(g) + 1/2 O2(g) is 6.66 x 1012 at 1000 K. Calculate K at 1000 K for the reaction: 2 CO(g)+ O2(g) 2 2 CO2(g).

A 9.40 L reaction vessel at 491°C contained 0.186 mol H3, 0.785 mol I3, and 2.81 mol HI. Assuming that the substances are at equilibrium, find the value of K. at 491°C for the reaction of hydrogen and iodine to give hydrogen iodide. The equation is H2 (9) + 1(9) = 2HI(9) K. =

Calculating an equilibrium constant from a partial equilibrium composition Ammonia will decompose into nitrogen and hydrogen at high temperature. An industrial chemist studying this reaction fills a 25.0 L tank with 2.4 mol of ammonia gas, and when the mixture has come to equilibrium measures the amount of hydrogen gas to be 0.36 mol. Calculate the concentration equilibrium constant for the decomposition of ammonia at the final temperature of the mixture. Round your answer to 2 significant digits. K = x10 × Ś olo 18 Ar 8.

General Chemistry 4th Edition McQuarrie Rock Gallogly University presentedi The equilibrium constant for the chemical equation N,(g) + 3 H, (g) =2 NH,(g) is K, = 0.139 at 237 °C. Calculate the value of K. for the reaction at 237 °C. Ke =