LISTA DE EXERCÍCIOS AULA 06/10/2016

Similar documents
TYPES OF CHEMICAL REACTIONS

Chapter 4 Reactions in Aqueous Solutions. Copyright McGraw-Hill

Unit 6 ~ Learning Guide Name:

CH 221 Chapter Four Part II Concept Guide

Chapter 4. Types of Chemical Reactions and Solution Stoichiometry

Ch 8 Practice Problems

Ch 4-5 Practice Problems - KEY

During photosynthesis, plants convert carbon dioxide and water into glucose (C 6 H 12 O 6 ) according to the reaction:

Lecture 5. Percent Composition. etc. Professor Hicks General Chemistry II (CHE132) Percent Composition. (aka percent by mass) 100 g.

K P VERSUS K C PROPERTIES OF THE EQUILIBRIUM CONSTANT

Chapter 4 Types of Chemical Reaction and Solution Stoichiometry

5. [7 points] What is the mass of gallons (a fifth) of pure ethanol (density = g/cm 3 )? [1 gallon = Liters]

Chapter 3 Test Bank. d. The decomposition of magnesium oxide produces 2.4 g of magnesium metal and 3.2 g of oxygen gas.

Ch 9 Stoichiometry Practice Test

2. Relative molecular mass, M r - The relative molecular mass of a molecule is the average mass of the one molecule when compared with

26. N 2 + H 2 NH N 2 + O 2 N 2 O 28. CO 2 + H 2 O C 6 H 12 O 6 + O SiCl 4 + H 2 O H 4 SiO 4 + HCl 30. H 3 PO 4 H 4 P 2 O 7 + H 2 O

Topic 9: Acids & Bases

Name Class Date. volume of solution molarity of solution amount of solute in moles

Unit 4: Reactions and Stoichiometry

c. K 2 CO 3 d. (NH 4 ) 2 SO 4 Answer c

Name. Practice Test 2 Chemistry 111

4. A chemist mixes g of potassium permanganate, g of ethanol, and excess sulfuric acid. These chemicals react as follows:

Chapter 6. Chemical Reactions. Sodium reacts violently with bromine to form sodium bromide.

2. If a gas is released in a reaction (ex: Hydrogen gas bubbles off), is it written as a reactant or a product?

HOMEWORK 1C. (d) 2D + E 2F K eq = 1 x 10 9 I C E

General Chemistry 1 CHM201 Unit 2 Practice Test

Part One: Ions in Aqueous Solution

1. What is the mass percent of sulfur in Al 2 (SO 4 ) 3? A % C % B % D %

Problem Solving. Percentage Yield

Stoichiometry ( ) ( )

Chapter 4 Reactions in Aqueous Solution

1. Hydrochloric acid is mixed with aqueous sodium bicarbonate Molecular Equation

Ions in Solution. Solvent and Solute

Which of the following answers is correct and has the correct number of significant figures?

F321: Atoms, Bonds and Groups Group 7

3 Chemical Equilibrium

Reactions in Aqueous Solutions

Mr. Storie 40S Chemistry Student Acid and bases Unit. Acids and Bases

Unit Two Worksheet WS DC U2

is considered acid 1, identify the other three terms as acid 2, base 1, and base 2 to indicate the conjugate acid-base pairs.

Chapter 4. Reactions in Aqueous Solution

Page 1. Exam 2 Review Summer A 2002 MULTIPLE CHOICE. 1. Consider the following reaction: CaCO (s) + HCl(aq) CaCl (aq) + CO (g) + H O(l)

-a base contains an OH group and ionizes in solutions to produce OH - ions: Neutralization: Hydrogen ions (H + ) in solution form

Unit VI Stoichiometry. Applying Mole Town to Reactions

Final Exam Review Questions You will be given a Periodic Table, Activity Series, and a Common Ions Chart CP CHEMISTRY

Gas Laws. Bonding. Solutions M= moles solute Mass %= mass solute x 100. Acids and Bases. Thermochemistry q = mc T

2. Write a balanced chemical equation which corresponds to the following equilibrium constant expression.

Unit Nine Notes N C U9

C. Perform the following calculations and Round into correct scientific notation.

Sample Problem Set. Teacher Notes and Answers. Skills Worksheet PERCENTAGE YIELD. Name: Class: Date:

Chapter 4. The Major Classes of Chemical Reactions 4-1

C2.6 Quantitative Chemistry Foundation

Chemical Reactions. Chemical changes are occurring around us all the time

Exam #5 May 2, Closed Book Exam - No books or notes allowed. All work must be shown for full credit. You may use a calculator.

2) Isotopes are atoms of the same element, which have the same number of but a different number.

APC Spring Break Take-Home Exam Instructions

Solubility Rules See also Table 4.1 in text and Appendix G in Lab Manual

4.6 Describing Reactions in Solution

Chapter 9. Table of Contents. Stoichiometry. Section 1 Introduction to Stoichiometry. Section 2 Ideal Stoichiometric Calculations

For Practice 4.1 Magnesium hydroxide, the active ingredient in milk of magnesia, neutralizes stomach acid, primarily HCl, according to the reaction:

Exam 1, Ch October 12, Points

Chemistry 20 Lesson 36 The Whole Enchilada

1. How many significant digits are there in each of the following measurements? (½ mark each) a) ha b) s. c) d) 0.

How many carbon atoms are in 1 mol of sucrose (C 12 H 22 O 11 )? A) 7.23 x B) 6.02 x C) 5.02 x D) 12 E) 342

Chemistry 2202 Stoichiometry Unit Retest Review Guide

Chp 13, 14, 15 SHOW ALL WORK AND CIRCLE FINAL ANSWERS. a) 1 only b) 2 only c) 3 only d) 1 and 2 only e) 1, 2, and H 2

AP Chapter 15 & 16: Acid-Base Equilibria Name

EXAM REVIEW. a b c d What would be the mass of mol of sulfuric acid?

4. Magnesium has three natural isotopes with the following masses and natural abundances:

Unit 3: Chemical Equilibrium Chemistry Write balanced chemical equations for each of the following. Pay close attention to the physical states!

Chapter 5 Chemical Calculations

... [1] (ii) Draw a dot-and-cross diagram to show the bonding in NH 3

F321: Atoms, Bonds and Groups Moles and Equations

1. Determine the mass of water that can be produced when 10.0g of hydrogen is combined with excess oxygen. 2 H 2 + O 2 2 H 2 O

Funsheet 9.1 [VSEPR] Gu 2015

Topic 1 Review. Ms. Kiely Coral Gables Senior High IB Chemistry SL

1. Complete an Initial/Change/Final molarity table for each. (a) A + 2B C (b) 3D + E 2F I I

NCERT Solutions for Atoms and Molecules

Chemistry 101 Chapter 4 STOICHIOMETRY

UNIT 2. Chemical Reactions. Chapter 4: Developing Chemical Equations. Chapter 5:Classifying. Chemical Reactions. Chapter 6:Acids and Bases

Chapter 6. Types of Chemical Reactions and Solution Stoichiometry

AP Chemistry Summer Assignment

Chapter 8. Chemical Equations. Flames and sparks result when aluminum foil is dropped Into liquid bromine.

Stoichiometry. Consider the reaction in which the reactants are nitrogen gas and hydrogen gas. They produce the product ammonia gas.

AP Chemistry Summer Assignment

Chemical Reaction Defn: Chemical Reaction: when starting chemical species form different chemicals.

CHAPTER 9 CHEMICAL QUANTITIES

Aqueous Reactions and Solution Stoichiometry (continuation)

Unit 4a: Solution Stoichiometry Last revised: October 19, 2011 If you are not part of the solution you are the precipitate.

Write equilibrium law expressions from balanced chemical equations for heterogeneous and homogeneous systems. Include: mass action expression.

Chemical Reactions: An Introduction

Chem II - Wed, 9/14/16

Name: Unit 9- Stoichiometry Day Page # Description IC/HW

Compounds in Aqueous Solution

X Unit 15 HW Solutions Acids & Bases. Name:

Unit 7: Stoichiometry Homework Packet (85 points)

Empirical formula C 4 H 6 O

(DO NOT WRITE ON THIS TEST)

CHEM 200/202. Professor Jing Gu Office: EIS-210. All s are to be sent to:

UNIT 3 IB MATERIAL BONDING, MOLES & STOICHIOMETRY

Transcription:

LISTA DE EXERCÍCIOS AULA 06/10/2016 1- Sodium hypochlorite, the active ingredient in Clorox, can be made by the following reaction: 2 NaOH(aq) + Cl 2 (g) NaCl(aq) + NaClO(aq) + H 2 O(l) If chlorine gas is bubbled continuously through a solution containing 60.0 g of NaOH, how many grams of NaClO can be produced, assuming the reaction goes to completion? 2- For the following unbalanced chemical equation: NiS + O 2 + HCl NiCl 2 + H 2SO 4 a) Write the balanced chemical equation for this reaction. b) What mass of NiCl 2 will be produced if 0.458 g of NiS reacts? 3-Vanadium (V) oxide, V 2 O 5, can be reduced by zinc to form vanadium (II) oxide, V 2 O 2 and zinc oxide, ZnO. a) Write and balance the chemical equation for this process. b) What mass of vanadium (II) oxide can be produced from a mixture of 100.0 grams of V 2 O 5 and 100.0 grams of Zn? 4- Many binary compounds of phosphorus and sulfur have been prepared. Balance the following chemical equation for the preparation of P 4 S 5. (Hint: balance the S first.) P 4 S 3 + Br 2 P 4S 5 + PBr 3 What is the maximum quantity of P 4 S 5 that could be prepared from 100.0 g of P 4 S 3 and 100.0 ml of liquid bromine? (Density of bromine is 3.12 g/ml) 5- A 10.0 ml sample of concentrated sulfuric acid contains 17.7 g of H 2 SO 4. Determine the molarity of concentrated sulfuric acid. 6- Pure acetic acid (C 2 H 4 O 2 ) has a density of 1.049 g/ml. Calculate the molarity

of pure (anhydrous) acetic acid. 7- A hydrochloric acid solution is prepared by dissolving 1.97g of hydrogen chloride gas in 27.3 ml of water and then diluting that mixture to a total volume of 250.00 ml. Calculate the molarity of the resulting solution. 8- The concentration of NaClO in Clorox is 0.705 M. Calculate the mass of NaClO present in 1.0 ml of Clorox. 9- A solution is prepared by dissolving x grams of potassium nitrate in water and diluting to a total volume of 100.0 ml. Another solution is prepared by dissolving y grams of sodium chloride in water and diluting to a total volume of 500.0 ml. Both solutions are then mixed together, giving a final concentration of KNO 3 of 0.073 mol/l and a final concentration of NaCl of 0.128 mol/l. Calculate x and y. 10- The toxic compound NCl 3 can be formed from the reaction of bleach (NaClO) with ammonia (NH 3 ): NaClO(aq) + NH 3 (aq) NCl 3 (l) + NaOH(aq) a) Write a complete, balanced, net ionic equation for this process. b) You accidentally pour 1.0 ml of Clorox into a large bucket of ammonia solution. What mass of NCl 3 can be produced if the reaction goes to completion? (Clorox is a 0.705-molar solution of NaClO in water.) 11- A sample of calcium carbonate weighing 6.35 grams is placed in 500.0 ml of 0.31M hydrochloric acid and allowed to react to form calcium chloride and carbon dioxide gas. Calculate the maximum mass of carbon dioxide gas that can be produced. 12- What volume of 0.0843 mol/l Ba(OH) 2 neutralize a 1.00-mL sample of 12.0 mol/l acetic acid? would be required to completely

13- A student has dissolved 87.5 grams of sodium hydroxide in 1.53 liters of water. This strongly basic solution must be neutralized before disposal. What volume of 1.27 mol/l HCl would be required to completely neutralize this solution? 14- Phosphoric acid can be neutralized by sodium hydroxide according to the equation: H 3 PO 4 + 3 NaOH Na 3PO 4 + 3 H 2 O a) What volume of 0.176 M NaOH would be required to neutralize 5.00 ml of concentrated (14.8 M) phosphoric acid? 15- You are given 2.00 grams of a white solid and told that it is a mixture of NaCl and Na 2 CO 3. You dissolve the sample in water and titrate with HCl; complete neutralization requires 23.0 ml of 1.00 mol/l HCl: Na 2 CO 3 + 2 HCl H 2CO 3 + 2 NaCl Calculate the mass of Na 2 CO 3 in the unknown sample. 16- The equation: N 2 O 4 (g) 2 NO 2 (g) has an equilibrium constant K C of 6.1 10-3 at 25 C. Calculate the equilibrium constant for the related reaction: NO 2 (g) ½ N 2 O 4 (g) 17- Nitrogen oxides are partly responsible for smog. Nitrogen monoxide, NO, is released from the burning of fossil fuels, and is oxidized by oxygen in the air to form brown nitrogen dioxide, NO 2 : 2NO(g) + O 2 (g) 2NO 2 (g) K P = 2.4 1012 at 25 C a) Calculate the value of K c for this reaction at 25 C. b) On a certain day, the partial pressures of NO, O 2, and NO 2 were as follows: P = 152 torr; P = 1.1 O2 NO 10-5 torr; P = 3.6 10-5 NO2 torr. Calculate the value of Q, and determine if NO 2 will be produced or consumed under these conditions.

18- The decomposition of NOBr has an equilibrium constant K P = 0.028 at 350 K: NOBr(g) NO(g) + ½Br 2 (g) a) Calculate the value of K c for this reaction at 350 K. b) A 2.00-liter flask contains 0.50 mol NOBr, 0.40 mol NO, and 0.20 mol Br 2 at 350 K. Calculate the reaction quotient Q, and determine if NOBr will be produced or consumed under these conditions. 19- Consider the decomposition of SO 2 Cl 2 at 600 K. SO 2 Cl 2 (g) SO 2 (g) + Cl 2 (g) ΔH = +67 kj/mol Predict the change in SO 2 Cl 2 concentration at equilibrium if you: i) add more SO 2 ; ii) decrease the volume of the flask iii) raise the temperature 20- In an investigation of the reaction: CO 2 + H 2 CO + H 2 O a chemist put 0.50 mol CO 2 and 0.50 mol H 2 into a 2.00 L flask and allowed them to reach equilibrium at 690 K. At equilibrium 0.38 mol CO 2 remained. What is the equilibrium constant for this reaction at 690 K? 21- Consider the equilibrium decomposition of SO 2 Cl 2 at 600 K: SO 2 Cl 2 (g) SO 2 (g) + Cl 2 (g) K C = 6.1 at 600 K A 1.00-liter evacuated flask is filled with 0.183 moles of SO 2 Cl 2 Calculate the moles of each gas at equilibrium, and the total pressure. at 600 K. 22- For the following Bronsted-Lowry acid-base reactions, identify the reactant which is acting as an acid and the reactant acting as a base: HN 3 + NH 2OH NH 3 OH + - + N 3 CN - + B(OH)3 HCN + BO(OH) 2 - Si(OH) 4 + C 6H 5 O - - SiO(OH)3 + C6 H 6 O

23- Calculate the ph of each of the following solutions. a) 0.027 M KOH b) 0.020MHBr c) 1.0 10-3 mol/l Ba(OH)2 d) 1.0 10-9 mol/l KOH 24- A solution is prepared by mixing 500. ml of 0.10 M NaOH with 500. ml of 0.0400 M H 2 SO 4. a) Write the equation for the chemical reaction which will take place. b) Calculate the ph of the resultant solution. 25- Calculate the ph of a 0.100 M solution of HF (K a = 6.8 10-4 ) 26- Calculate the ph of a 0.0500 M solution of HIO 3. (K a = 1.69 10-1 ) 27- Calculate the ph of a 0.117 M solution of CH 3 NH 2. (K b = 4.3 10-4 ) 28- Many home pools are disinfected by adding calcium hypochlorite, Ca(OCl) 2. The hydrolysis of the hypochlorite ion yields hypochlorous acid. Given that K a for HOCl = 3.0 10-8, calculate the ph of an 0.100 M solution of calcium hypochlorite, Ca(OCl) 2.

2024 © sciencedocbox.com Privacy Policy | Terms of Service | Feedback