Equilibrium Questions and Answers

If 15 0 grams of sodium metal are thrown into water how many grams of hydrogen gas will be produced

32 This graph represents the decay of a radioactive Isotope What is its half life Mass of a Radioisotope g 33 Consider the reaction Time hours A 2 hr B 3 hr C 4 hr D 6 hr 2SO 8 2SO 8 O 8 for which K 3 6 at a given temperature A 1 0 L flask at that temperature initially contains 2 0 mol SO 4 0 m SO and 0 50 mol O As equilibrium is established at that temperature the concentration of O A will de

The reaction X g Zg has an equilibrium constant of 2 5 Which picture best illustrates an equilibrium mixture A C O O B D O KEY O X O Z O

The weak base ionization constant Kb for HCO3 is equal to

How many moles of nitrogen would it take to produce 25 0 grams of NH3 N 3H 2NH

The chemical equation below shows a reaction at equilibrium N g 3 H g 2 NH3 g Which change in the reaction will occur if additional nitrogen N is added O The concentration of H will increase The concentration of NH3 will decrease The equilibrium will shift to the left and form more reactants The equilibrium will shift to the right and form more products O

Given the following chemical equation CaO s CO2 g If the above reaction has just reached equilibrium which statement about the reaction must be true O The mass of CO2 is equal to the mass of CaCO3 O The mass of CO2 is equal to the mass of the CaO The CaCO3 has been completely converted into CaO and CO2 O The rate at which CaCO3 is decomposing is equal to the rate at which it is forming CaCO3 s

Exercise 1 Using the ion product of water for calculations giv Calculate OH when the H3O has the following values ulay Hq privolic 1 0 x 10 7 M H3O 1 0 x 10 11 M H3O 1 0 10 5 M H3O 2 8 x 10 10 M H3O 8 6 x 10 4 M H3O dib flow aged Am 1st Einsat NE 15 12 183310 802 ahlend

Exercise K Calculating pH Calculate the pH of the following solutions at 25 C Indicate whether the solution is acidic basic or neutral Be sure to notice whether the H3O or OH is given A solution is considered neutral ONLY if pH is exactly 7 0 pH to Vy H3O 1 0 x 10 6 M H3O 2 5 x 10 3 M OH 1 0 x 10 5 M OH 2 0 x 10 M OH 5 6 x 10 5 M Tap Acidic Basic or Neutral ABN ABN ABN ABN ABN

Calculate the heat energy released when 22 4 g of liquid mercury at 25 00 C is converted to solid mercury at its melting point Constants for mercury at 1 atm heat capacity of Hg 1 melting point enthalpy of fusion 28 0 J mol K 234 32 K 2 29 kJ mol qp kJ

A buffer solution contains 0 25 M CH COOH and 0 56 M CH C00 What is the pH of this solution 3 5 K 1 8 x 10 for CH COOH a CH3COOH CH3COO H

Rank the following from most to least acidic Lemons pH 2 Seawater pH 8 Grapefruit pH 3 Urine pH 6 Salvia pH 7 Vinegar pH 5 Tomato juice pH 4 Oven Cleaner pH 13 Gastric Acid pH 1 Soap pH 12

19 Calculate the pH for the following 1 x 10 8 a b C d e 1x 10 7 1 x 10 3 1x 10 12 1 x 10 4

If I have 128 grams of O gas at a pressure of 5 6 atm and a volume of 12 liters what is the temperature 306 K 6 4 K 205 K 155 K

Part 1 Lightning Round 6 pts each Consider the condensation of water H O g H O 1 What are the signs of AH and AS What is the temperature dependence of AG At what temperature is AG equal to zero

a Concentrations of rea b Forward and reverse rate of reaction is c Temperature has no effect on equilibrium d Equilibrium constant expression is equal to reactants over products 34 Given the following reaction 2H O 2H O what would the top part of the equilibrium constant expression look like a H O c H O 35 Using the reaction listed in 34 2H O 2H O determine H given Kc 0 51 H O 0 05M and 0 0 04M a 3 1M c 0 35M b H OP d H O a acid c neutral Chapter 14 Acids Bases 36 What color will phenolphthalein turn if it is added to a base a F H O C O H F b 5 1M d 0 12M b H F OH d F H O the H O 1 0x107M the solution is b White or clear a magenta pink c blue d yellow Determine the products of the following proton exchange reaction HF H O bochon b base 2181 101 ALS

15 Draw the pH scale Label with numbers and which side is acidic and which is basic

Essay 3 topic Explain in your own words what are conjugate acids and bases How can you organize different weak and strong acids in order of relative strength and what does this tell you about the relative strength of their conjugate bases

4pts 21 If you mixed one mole of hydrogen gas and one mole of halogen gas in a container and le come to equilibrium which of the reactions below would produce the most products a H F 2HF g K 4 7 x 10 Hw Cl 2HCl g K 8 6 x 10 b c H Br 2HBr g K 2 8 x 10 Hw 2HI g K 0 50 d e There is not enough information to decide

2 Balance the following equation H g N g NH3 g If the of all of the reactants and products is 2 0M what is Q If Keq 4 0 which way must reaction shift in order to reach equilibrium

1 Balance the following equation SO g O g SO3 g If the SO 8 0M the 0 6 0M and the SO3 10 0M what is Q If Keq 0 799 which side is favored reactants or product Which way must the reaction shift in order to reach equilibrium

Write the reaction out and see if the products will be soluble or will precipitate using your solubility chart Choose the reactants which when combined will produce a precipitate A NaC2H302 and HCI aq B KOH aq and Cd NO3 2 aq C AgNO3 aq and Ca C2H302 2 aq D NaOH aq and HCI aq

PC15 9 PCI 3 g Elinelid Cl g 2 If some phosphorus trichloride PCI3 is removed from the system then the equilibrium position would not be affected by such a change shift to the right in the direction of products shift to the left in the direction of reactants 4

The following reversible system is al 2 SO3 g 2 SO2 g O2 g If some sulfur trioxide SO3 is removed from the system then the equilibrium position would not be affected by such a change shift to the right in the direction of products shift to the left in the direction of reactants 4

1 6 After Procedure Step S the solution in Well A1 was in equilibrium What happened to the solution in Well A1 during Procedure Step 5 Did the equilibrium shift Explain this on the basis of the Le Chatelier Principle

Combining aqueous solutions of Srl2 and Li2SO4 produces s a precipitate Which ion s is are spectator ions in the reaction A Sr2 only B Li only C Sr2 and SO42 D SO42 and l E Li and I

The PCI5 g PC13 g g Cl2 g If additional phosphorus pentachloride PCL5 is added to the system then the equilibrium position would not be affected by such a change shift to the right in the direction of products shift to the left in the direction of reactants 4

The follo CO g H O g H2 g CO2 g If additional carbon monoxide CO is added to the system then the equilibrium position would 4 not be affected by such a change shift to the right in the direction of products shift to the left in the direction of reactants

D1 C1 B1 7 A 8 A1 4 D5 C16 4 1 Z 2 3 Data Table 2a Effects of KI Concentration Trial KI HCI Starch H O Na S O drops drops drops drops drops s 4 5 6 7 123 8 8 8 8 8 8 8 86648 22 2 222 2 2 2 NNNNNNNN 2 2 2 2 2 2 2 2 2 Data Table 2b Effects of H O Concentration Trial KI HCI Starch H O Na S O H O drops drops drops mL drops mL 1 4 4 4 4 4 4 4 4 444 4 4 4 4 0 0 22 4 4 6 6 6 10 6 0 0 0 1 0 1 0 2 0 2 0 3 6 6 H O Time Time Average mL sec sec Time T sec 7 7 0 4 18 76 0 4 0 4 24 06 0 4 0 4 33 30 0 4 0 4 10 23 0 4 Rate 0 4 18 596 0 4 0 3 2421 0 3 0 2 31 50 0 2 0 1 1 08 1 T 19 345 25 20 34 485 90235 35 67 90 24 Calculate the rates plz Rate 1 Tag Time Time Average sec sec Time T sec 19 355 20 15 24 065 23 921 31 69 31 995 1 16 S

Enter your answer in the provided box Calculate the pH of an acetic acid acetate buffer in which the concentration of acetic acid is al 0 48 M but the concentration of sodium acetate NaCH3COO corresponds to the following va 0 58 M K for CH COOH is 1 8 10 5 Report your answer to three significant figures

What is the pH of the solution formed by mixing 300 0 mL of 0 10 M Ba OH 2 aq and 200 0 mL of 0 30 M HCl aq at 25 C 01 2 03 4 07 0 08 2

What is the theoretical pH of a 0 001 M KCl solution 0 001 11 CA

Commercial battery acid is 38 sulfuric acid H SO4 by mass and has a density of 1 29 g mL What amount of sodium hydroxide is required to neutralize 50 0 mL of battery acid The molar mass of sulfuric acid is 98 076 g mol O 0 25 mol O0 66 mol O 1 32 mol O 0 50 mol

A chemist dissolves 261 mg of pure perchloric acid in enough water to make up 130 mL of solution Calculate the pH of the solution Round your answer to 3 significant decimal places 0 X C

What is the theoretical pH of a 0 01 M HCl solution 14 12 02 the pH cannot be determined

What is the theoretical pH of a 0 01 M NaOH solution can not be determined 12 0 2 02 Question 4 What is the theoretical pH of a 0 001 M NH4OH solution 3 0 001 O 11

What is the theoretical pH of a 0 001 M HNO3 solution The pH can not be determined 0 001 14 0 3 07 011 03

lodine gas and hydrogen gas combine to form hydrogen iodide as shown below At 800 K the equilibrium constant Kc 64 0 12 g H g 2 HI g In an experiment 0 500 mol of H and 0 500 mol of 12 are mixed in a 1 00 L container What is the concentration of HI when the reaction reaches equilibrium 00 30 M O 0 40 M 1 60 M 0 80 M M

O Consider the reaction of H g F g 2 HF g What happens to the concentration of substance when a H2 is decreased b HF is decreased a F select and HF select and F select b H select

7 Be sure to answer all parts Calculate the equilibrium constant for the reaction using the balanced chemical equation and the concentrations of the substances at equilibrium Use the appropriate significant figures in reportin answers CO g H O g CO g H g CO 0 201 M H O 0 0204 M CO 0 139 M H 0 139 M

Be sure to answer all parts For each value are the reactants or products favored at equilibrium a K 2 0 108 Cool b K 0 0075

Be sure to answer all parts Write an expression for the equilibrium constant for the react 2 NO g O g 2 NO g

Be sure to answer all parts If a urine sample has a pH of 6 50 calculate the concentrations of H3O and OH in the sa H O X 10 select OH x 10 select M M

3 Given each equilibrium constant state whether the reactants are favored the products are favored neither is favored at equilibrium a 0 65 select b 54 select c 7 4 1012 select d 5 8 10 8 select

Consider the endothermic reaction 2 NH3 g 3 H g N g What effect does each of the follow changes have on the direction of equilibrium a decrease NH3 d increase temperature select b decrease N select c decrease H select e decrease temperature select f decrease pressure

1 Be sure to answer all parts Consider the following reaction a Write the expression for the equilibrium constant K CO g H O g CO g H g b Calculate K using the following concentrations of each substance at equilibrium CO 0 090 M H O 0 24 M CO 0 15 M H 0 60 M K Use significant figures in reporting your answer

Be sure to answer all parts For the pair of acids 1 Label the stronger acid 2 Give the formula for the conjugate b 3 Label the stronger conjugate base H PO4 phosphoric acid K 7 5 10 3 select or HCOOH formic acid K 1 8 10 4 select 7

Be sure to answer all parts Calculate the value of OH from the given H3O and label the solution as acidic or a 10 13 M x 10 select b 10 8 M x 10 M M

Use the data in the tables below to label the stronger acid in each pair Which acid in each pair has th stronger conjugate base a H O or HSO b HNO or HI 0 e HBr or HCI is the stronger acid Increasing acid strength is the stronger acid Increasing acidity is the stronger acid Table 9 2 Relative Strength of Acids and Their Conjugate Bases Conjugate Base Strong Acids Hydrolodic acid Hydrobromic acid Hydrochloric acid Sulfuric acid Nitric acid Acid Hydronium ion Weak Acids Phosphoric acid Hydrofluoric acid Acetic acid Carbonic acid Ammonium ion Hydrocyanic acid Water HI HBr HCI H SO HNO H O Hydrogen sulfate ion Phosphoric acid Hydrofluoric acid H PO HF CH COOH H C NH HCN H O has the stronger conjugate base has the stronger conjugate base Acetic acid Carbonic acid Dihydrogen phosphate ion Ammonium ion Hydrocyanic acid Bicarbonate ion Hydrogen phosphate ion has the stronger conjugate base IT Br CI HSO NO H O H PO F CH COO HCO NH CN OH Table 9 3 Acid Dissociation Constants K for Common Weak Acids Acid K 1 2 x 10 7 5 x 109 Structure HSO H PO HF lodide ion Bromide ion Chloride ion Hydrogen sulfate ion Nitrate ion CH COOH H C H PO NH HCN HCO HPO Water Dihydrogen phosphate ion Fluoride ion Acetate lon Bicarbonate ion Ammonia Cyanide ion Hydroxide ion 7 2 x 10 1 8 x 10 4 3 x 10 6 2 x 10 5 6 x 10 4 9 x 10 5 6 x 10 2 2 x 10 2 increasing base strength

Be sure to answer all parts Calculate the pH from each H O concentrat a 6 0 10 8 M b 4 5 x 10 3 M