Chapter 5 thermochemistry review

Chapter 5 thermochemistry review. Multiply (1) and (2) by the factor 3. 10 atm. - endothermic work (w) is positive when work is done on the system. mandracchiae2026. Hydrogen gas burns in air according to the equation below. E. Chapter 5 Thermochemistry ; Chapter 7; AP Chemistry Zumdahl 7E Chapter 16 Notes; AP Chem Brand Review Books. 37 Bomb calorimetry measures ∆H at a constant volume by measuring the ∆T of a solution with the reasoning ∆Hreaction = -∆HH2O. Chapter 5 will include the following topics: - Energy Chapter 5 Review. tomchoueifati. measure of the thermal energy within a sample of matter. Since heat is released from the reactant to the surroundings, the surrounding temperature is raised. Pre-Publication Material. Start studying CHEM200 Chapter 5- Thermochemistry- openstax. 50 moles of nitrogen at 23. Study with Quizlet and memorize flashcards containing terms like Energy, Work, Heat and more. • ∆E occurs with almost every chemical, physical, or nuclear CHEMISTRY 30 COURSE REVIEW Unit 1 – Thermochemistry. Reverse (1) and (2) so that reactants and products are on the same side as in the desired equation. The Chapter 5 packet can be found here:https://goo. Figure 5 Sliding a match head along a rough surface initiates a combustion reaction that produces energy in the form of heat and light. May 26, 2021 · About Press Copyright Contact us Creators Advertise Developers Terms Privacy Policy & Safety How YouTube works Test new features NFL Sunday Ticket Press Copyright Dec 12, 2023 · Study with Quizlet and memorize flashcards containing terms like the study of energy and its transformations, study of the relation between chemical reactions and changes in energy, the energy transformed between objects because of a difference in their temperatures and more. 13. 0 license and was authored, remixed, and/or curated by Mark Draganjac via source content that was edited to the style and standards of the LibreTexts Chapter 5 | Thermochemistry 233. the heat released or absorbed during a chemical reaction; equivalent to (h), the change in enthalpy. 3. Energy can be defined as the capacity to supply heat or do work. Step 2: Identify the equations that have reactants or products on the same side of the arrow as in the desired equation. The study of energy transformations that occur in a collection of matter. riding bike down a hill. This chapter introduces many of the basic ideas necessary to explore the relationships Heat review •Heat is transfer of randomkinetic energy from: •Stuff with higher K. 2 H₂ + O₂ → 2 H₂O + 285 kJ/mol. Sep 6, 2023 · Chapter 4 - Chemical Bonding and Molecular Geometry ; Chapter 5 - Advanced Theories of Bonding ; Chapter 6 - Composition of Substances and Solutions ; Chapter 7 - Stoichiometry of Chemical Reactions ; Chapter 8 - Gases ; CHEM 1212K. 18 J/°C·g. pdf AP Chemistry Unit 5 Review. Sum of all Kinetic and Potential energies of the components of the system. thermochemistry. 5 gram sample of a metal at a temperature of 425°C is placed in 1. it could be the gas inside of balloon. if within the chemical substances- called chemical potential energy. Text: Tro, Fridgen and Shaw, 3rd CE (Chapter 6) Problems: A. units: J/g°C. Solid and gaseous helium never exist in equilibrium with each other at any temperature or pressure. 39a Previous Answer Chapter 5 - Thermochemistry - Exercises - Page 205: 5. Step 2: Check the coefficients of all entities in the equations to see if any must be adjusted by a factor so as to be equal to the coefficients in the desired equation. to stuff with lowerK. relationship between chemical reactions and energy changes that involve heat. Chapter 9 -Thermochemistry ; Chapter 10 - Liquids and Solids ; Chapter 11 - Solutions ; Chapter 12 - Thermodynamics CHAPTER 5. 5 Energy Basics 5 Calorimetry 5 Enthalpy. 1: The Flow of Energy-Heat. We also assume that only the water is going to be heated. Units: J/g C. Relation to amount of heat (q) where q is heat, m is mass, s is specific heat and T = change in temp ( T = Tfinal Tinitial) • Heat capacity (C) - the amount of heat required to raise the temp of an object by. 3) energy is released as new bonds form. 5K plays. Chapter 17 Review. Going Solo. Energy used to cause an object with mass to move against a forcew= F x d. 8 kJ/mol at 298 K. Hess' Law Handout. calculate Q of water using Q = mc∆T. Thermal energy measures the total amount of energy in a substance. = 101. 9 terms. 08206 Latm (mol. energy change = heat + work heat (q) is positive when heat flows into the system. Textbook Authors: Zumdahl, Steven S. Click the card to flip 👆. • Chemistry is the study of matter: it’s properties, interactions, reactions, and ENERGY CHANGES. 184 and more. The contents in the container become hot. 5 - 5. Chemistry Module 5. 1; ECO 201 - Chapter 2 Thinking like an economist part 2; A&P II Chapter 21 Circulatory System, Blood Vessels; Untitled document - WRD 111 Professor Parsons; Chapter 5 Lecture notes; COM 315 Exam Two Study Guide Fall 2019; Physio Ex Exercise 4 This chapter focuses on thermochemistry, which is the study of the thermal energy associated with chemical and physical changes of substances. 26. Thermochemistry heat changes that chemical reactions. Exothermic Reaction. Exercise 135a. the study of heat effects in chemistry. ice cube melts and cools surroundings = + (system gain heat = icecube gains heat) steam condenses on skin, causing a burn = - (system loses heat - condensing steam is system) reaction produces 1422 J => q = -1422 J. Mar 13, 2023 · What is ∆H when 5. relationships between chemical reactions and energy changes that involve heat. 8th - 10th. the transformations of energy - especially heat - during chemical reactions. The reaction is exothermic since it releases energy. molar heat capacity. Law of Conservation of Mass. View all notes for Science Form 3. If the solution is water: c (H2O) = 4. Sep 25, 2016 · This video explains the concepts from your packet on Chapter 5 (Thermochemistry), Sections 5. thermal energy is related to temperature and associated with kinetic energy of molecules. 2. We assume that the density of water is 1. Page 839: Standardized Test Prep. , ISBN-10: 1133611095, ISBN-13: 978-1-13361-109-7, Publisher: Cengage Learning Thermochemistry (chapter 5) • Is the study of the energy changes that accompany physical and chemical changes. You will find useful examples, diagrams and equations to help you master the concepts and calculations. Since we are interested in reversing the reaction using only one-half of the. Exercise 134c. When a system undergoes a change the change in internal energy, ∆E is defined as the heat, q, added to the system, plus the work, w, done on the system by its surroundings: ∆E= q + w. 11. 4 ° C. First Law of Thermodynamics - the energy of the universe is constant. Calculate the change in internal energy, Δ U of a system if it: (a) absorbs 405 J of heat and does 760 J of work on the surroundings. 54 L to 5. (Choice C) Chemistry 9th Edition answers to Chapter 6 - Thermochemistry - Review Questions - Page 284 9 including work step by step written by community members like you. 1 Sliding a match head along a rough surface initiates a combustion reaction that produces energy in the form of heat and light. work. Section 11. Terms in this set (120) Thermodynamics. 5 The Nature of Chemical Energy A. Sep 30, 2016 · This video explains the concepts from your packet on Chapter 5 (Thermochemistry), Sections 5. Step 3: Add equations (4), (5), and (6), and their changes in enthalpies. 15 Qs. SP-ecific Heat of Water CalorimetrY. Answers for chapter 5 review 1-20. About Press Copyright Contact us Creators Advertise Developers Terms Privacy Policy & Safety How YouTube works Test new features NFL Sunday Ticket G. Types of Chemical Reactions. K) 1 cal-4. Feb 21, 2019 · General Chemistry I (CHEM 1311) Instructor: Science and engineering majors study atomic structure, chemical reactions, thermodynamics, electron configuration, stoichiometry, chemical bonding, molecular structure, gases, and states of matter. Thermochemistry. Chemistry: The Central Science. PE: from IMF [5. Learn. Aug 26, 2023 · 5: Thermochemistry. Unit 5: States of Matter Unit 6: Kinetics & Equilibria Unit 7: Electro & Thermo Chemistry Unit 8: Materials. State Function. Exercise 2. Releases heat. The forms of energy that are chemistry related include: • During chemical reactions, chemical energy may be stored, released as heat, or converted Subject Guides. 34 A 47. product, we only need one-half the quantity of energy released. 35 mol of CO 2 reacts with excess MgO? What is ∆H when 35. SPM Chemistry Form 5 Chapter 2 – Carbon Compounds. What would likely happen (how would it feel) if you were to touch the flask in which an endothermic reaction were occurring? Standard conditions of temperature and pressure for a thermochemical equation are __ and __kPa. 0: Introduction. E: Thermochemistry (Exercises) Page ID. Describes the heated associated with a rxn. Chapter 17: Thermochemistry 17. 4K plays. What are the three steps of a chemical reaction? 1) energy is needed (absorbed) to break bonds. matter that is being observed. PDF. 390 J/g °C; (b) Copper is a likely candidate. measure then calculate T final - T initial = ∆T. Next Answer Chapter 5 - Thermochemistry - Exercises - Page 205: 5. 5th - 6th. 0 metric ton of coal (assuming pure carbon) to gaseous carbon. Chemistry 1220 Chapter 6 Review: Thermochemistry. 3 Enthalpy. 2 Calorimetry. 1 Energy Basics. • Energy is defined as the ability to do work or the capacity to produce change. Energy Transformations. 1 / 28. Unit 1: Atomic Theory Unit 2: Molecular Structure Unit 3: Stoichiometry Unit 4: Thermochem & Gases. by Brown, LeMay, Bursten, Murphy, and Woodward. second law of thermodynamics. – The nutritional Calorie (capital C), Cal = 1,000 cal = 1 kcal – Wheaties that provides 100 nutritional Cal really gives 100 kcal or 100,000 cal . (credit: modification of work by Laszlo Ilyes) Chapter Outline. 11 u]? The specific heat of water is 4. hint for calorimetry: temp change. Calculate the specific heat capacity of a piece of wood if 1500. weightless, odorless, tasteless. = −129. These are homework exercises to accompany the Textmap created for "Chemistry: The Central Science" by Brown et al. Key Equations; Audio Glossary Math Review Home > > Chapter 6. 7. We will investigate the energy changes that take place during phase changes and the chemical reactions you have A greater attraction (lower Eel) Protons and electrons farther apart with a greater separation have. 0 g of the wood absorbs 67,500 joules of heat, and its temperature changes from 32°C to 57°C. states that if the mechanical energy of a system is constant, the increase in the thermal energy of the system equals the sum of the thermal energy transferred into the system and the work done on the system. Energy. Using the average fuel values of these substances, estimate the fuel value (caloric content) of this serving. measure the mass of water. Chapter 5 Thermochemistry. In chemistry, work is expansion or compression. Quick Notes. Study with Quizlet and memorize flashcards containing terms like Cancro (2014-2015) Learn with flashcards, games, and more — for free. , ISBN-10: 1133611095, ISBN-13: 978-1-13361-109-7, Publisher: Cengage Learning. K) 0. Password. Exercise 135b. 16 terms. Introduction Question: CHEM 101 Worksheet, Chapter 6: Thermochemistry Multiple choice questions 1-10 (page 1): circle the correct answer (-E) Show your work questions 11-13 (pages 2-3): give the complete answer in the space provided R-8. Dec 21, 2011 · Energy Level Diagram. 5 g of CO 2 reacts with excess MgO? This page titled Thermochemistry (Worksheet) is shared under a CC BY-NC-SA 4. Chem 101 DE - Chapter 9 Test. Part 3: Thermochemical Equations & Enthalpy Diagrams 1. The unit is then kJ/mol. 2 H₂O + 285 kJ/mol → 2 H₂ + O₂. energy used to cause temperature of an object to increase. 1 C. 2: Enthalpy and Reactions. SPM Form 5 Chemistry Chapter 5 – Chemical for Consumers. capacity to do work or transfer heat. •When faster atoms/molecules hit slower ones: •The faster ones get slower and the slower get faster. amount of energy required to raise temp of 1 mol of substance by 1⁰C. energy used to cause an object to move against a force. 0 o C under constant pressure of 1. Most of the energy used in our daily lives come from chemical reactions. A reaction that releases heat to the surroundings. Definition of work: w = F * d 7. It provides a list of formulas and equations that you need to know as well as the appropri energy required to raise the temp of 1g of substance by 1⁰C. B. 18 J/gºC. 0: Prelude to Thermochemistry Useful forms of energy are also available from a variety of chemical reactions other than combustion. We can measure energy changes in chemical reactions to help determine exactly what is happening and how it is occurring. 00 liters (1000 grams) of water which had an initial temperature of 18°C. supplying heat. 5 °C. calorimetry equation. principles is essential for chemists, physicists, biologists, geologists, every type of engineer, and just about anyone who studies or does any kind of science. 1. Surroundings can exchange energy and matter if the system is open or only energy if the system is closed. MC Chap 5. What is bond enthalpy? Study with Quizlet and memorize flashcards containing terms like Exothermic, Endothermic, 4. energy of motion, ex. energy. 184 J/g × K. We'll cover everything from nomenclature to energy to significant figures. Chapter 5. Exercise 136b. Heat measures the flow of energy from substances at high temperatures to those at low temps. the part of the universe that we are focusing on (the reaction) define "surroundings" in terms of thermochemistry. Chapter 5, 11, and 19 - Thermochemistry. Heat of Reaction. 1 Energy Changes in Chemical Reactions. it could be the amount of solute and solvent used to create a solution. Define energy as it relates to chemical systems. w. E = work + heat B. 1 3. a property of a system that is determined by specifying the systems conditions. One type of work (w) is the process of causing matter to move against an Terms in this set (41) Thermodynamics. Chemistry 9th Edition answers to Chapter 6 - Thermochemistry - Exercises - Page 289 73 including work step by step written by community members like you. Feb 13, 2023 · The initial temperature of the water was 22. Capability do work and transfer heat 2. Chapter 22. 15 °C. What is. Energy required = 7. Complementary General Chemistry – amount of energy required to raise the temperature of 1 g of water from 14. A general chemistry Libretexts Textmap organized around the textbook. AP Chemistry - Chapter 5 (Thermochemistry) Review. H. Thermodynamics: the study of energy and its transformations. 5 °C to 15. 314 J/mol. The Nature of Energy Energy is the capacity to work or transfer heat. 41a Answers for chapter 5 review 1-20. 47 kWh. the capacity to do work or transfer heat. Chemical Energy is Mainly Potential Energy One of the most important form of potential energy in molecules is electrostatic potential energy Reminder: the unit of energy commonly used is the Joule: An editor will review the submission and either publish your submission or provide feedback. Describe potential energy at the atomic-molecular level as energy stored by a system of interacting atoms or molecules based on their charges and the distance between them. Introduction. Study with Quizlet and memorize flashcards containing terms like thermochemistry, work, energy and more. Unit 3 Chem Test. kinetic energy. For example, the energy produced by the batteries in a cell phone, car, or flashlight results from chemical reactions. THERMOCHEMISTRY. 1 - 5. Chapter 20. Useful forms of energy are also available from a variety of chemical reactions other than combustion. 7. namic Equation Sheet 1 Bomb CalorimetrY. 2 2. Calculate the heat effect (in kJ) when 112 g of iron (es Aug 8, 2014 · Chapter 17 Review “Thermochemistry”. 1 & 17. The chapter presents enthalpy, the primary quantity by which we deal with heat in chemistry. 184J 0 °C -273 K 1. 2) Molar Enthalpy, ∆Hx = the enthalpy change per mole of a substance, where x indicates the type of change. Chapter Review. s m 1J = 1kg ⋅ 1 cal = 4. 13 Qs. haileyhascatz. dioxide releases 3. (Choice B) Solid and gaseous helium never exist in equilibrium with each other at any temperature or pressure. Equation to find final temperature. ∆H= mC∆T. Thermochemistry- Chapter 5 Review - Chemistry is the study of matter and the changes it undergoes Chemical and physical changes are always accompanied by energy and heat changes. Reverse the sign of ΔH. Endothermic. Test. There is no exchange with an isolated system. the rest of the universe (area around the reaction) define "state of a system". 15 J/°C · mol. KE: from VRT — temperature. Chapter 5: Thermochemistry. The quantity of heat, in joules or calories, required to raise the temperature of 1 gram of a substance 1 degree Celsius. Add Source or PDF Show Tags. Find step-by-step solutions and answers to Chemistry, AP Edition - 9781305957732, as well as thousands of textbooks so you can move forward with confidence. Chap 5 Worksheets Answers. The laboratory includes appropriate experiments. Exercise 1. Energy - capacity. P-es of Molecular EnergY. Chapter 19 - Chemical Thermodynamics. Match. . About Chapter 5: Homework Questions Review: Problem Solving Videos Optional: The following videos are the same as the ones presented earlier in the main text IY. Chem Exam 4 (Chs. This chapter introduces many of the basic ideas necessary to explore the relationships between chemical changes and energy, with a focus on thermal energy. It discusses heat and heat capacity, and the heat of chemical and physical changes. 4. ECO 201 - Chapter 2 Thinking like economist part 1; IS2080 - Chapter 2 Practice; BANA 2082 - Chapter 2. DankoK18. Calculate the amount of heat, in kJ, that is released when A. (2011A, 4 points total) 2 H2(g) + O2(g) ® 2 H2O( ) Calculate the standard enthalpy change, ∆ , for the reaction represented by the equation above. Chapter 18. Breaking and Formation of Chemical Bond. Students also viewed. What is the specific heat capacity of the metal if the final temperature of the metal and water at equilibrium is 21°C? (The specific heat capacity of water is 4. 184J Chapter 6: Thermochemistry In this Chapter: Textbook Resources. 2 Spontaneous Processes and Entropy and the Second Law of Thermodynamics The first Law of Thermodynamics states that energy is neither created nor destroyed; it is constant in the universe. gl/W Specific heat (s) - the amount of heat required to raise the temp of 1 g of a substance by 1 C. q=∆H. zvneumann21. Spring 2023 Semester CHEM 101 General Chemistry A Chapter 5: Thermochemistr. Heat. Chemistry the Central Science. define "system" in terms of thermochemistry. Energy is defined as the capacity to do work or transfer heat. Created by. • Thermochemistry -- aka Chemical Thermodynamics -- heat & energy flow. Complete combustion of 1. the change in internal energy of the system (in J)? 2. , ISBN-10: 1133611095, ISBN-13: 978-1-13361-109-7, Publisher: Cengage Learning What is thermochemistry? study of chemical reactions and energy changes that involve heat. 3 X 1010 J of heat. Tf= Q/ (cp) (m) + Ti. With this review, you'll be more than ready to tackle AP Chemistry! thermochemistry. extrapolate the line (check the figure below) . Amount of energy required to raise the temperature of one gram one unit Kelvin. Heat of Neutralization. Absorbs heat. All notes this chapter. This chapter introduces many of the basic ideas necessary to explore the relationships between chemical Chapter 5 Thermochemistry 5-1 5-1 Chapter 5: Thermochemistry Chapter In Context In this chapter we begin an exploration of thermochemistry, the study of the role that energy in the form of heat plays in chemical processes. Types of Energies ↓ 5. gl/W Jul 17, 2016 · This chemistry video lecture tutorial focuses on thermochemistry. FORM 3 CHAPTER 5: THERMOCHEMISTRY quiz for 9th grade students. These are things that you should have memorized to succeed in AP Chemistry. Enthalpy. A system receives 425 J of heat and delivers 425 J of work to its surroundings. Thermochemistry: the relationship between chemical reactions and energy changes. 5: Thermochemistry (Calorimetry) Now, Let’s quickly review a few definitions we will need to use in this section. energy change= mass (g)*specific heat*change in temperature. Chapter 9. Thermochemistry: study of the energy change associated with chemical reactions. heat. Chapter 21. Forgot Password. Science An Atoms First Approach. 8-9) 22 terms. Jun 16, 2022 · 5. Calculate q, w, and Δ E in kJ for the nitrogen gas in the balloon if its heat capacity is 29. When this reaction occurs, the reactant will lose heat to the surroundings. ? Chemistry 9th Edition answers to Chapter 6 - Thermochemistry - Review Questions - Page 284 7 including work step by step written by community members like you. System: object being investigated (= reaction mixture in thermochemistry) Surroundings: everything else. 7 kJ. Study with Quizlet and memorize flashcards containing terms like Thermodynamics, ThermoChemistry, Energy and more. Q-Chat. (a) A 28-g (1-oz) serving of a popular breakfast cereal served with 120 mL of skim milk provides 8 g protein, 26 g carbohydrates, and 2 g fat. On the basis of this experiment, what is the heat of solution per mole of KNO 3 [f. first law of thermodynamics. Study with Quizlet and memorize flashcards containing terms like Thermodynamics, Thermochemistry, Kinetic energy and more. Preview. An editor will review the submission and either publish your submission or provide feedback. Learn vocabulary, terms, and more with flashcards, games, and other study tools. the total amount of reactants and products in a chemical reaction. 5 - part 2 review. Do you want to learn more about the chemistry of gases, liquids, solids and solutions? Check out this pdf file from Michigan State University, which covers the topics of Chapter 5 in CEM 151 course. Types of Energy changes in a chemical system – temperature, phase, chemical, and nuclear -are they potential or kinetic -their formulas -what type of bonding is changing Terms Chapter 11:Thermochemistry-Heat and Chemical Change. (3) N2(g) + H2(g) → NH3(g) ∆H = –46 kJ. 1 kg m^2/s^2. Specific heat describes the amount of energy needed to change the Chapter 5 Thermochemistry Answers. ThermodY. Joule (J) 1 J =. ; Zumdahl, Susan A. Therefore, to reverse the reaction, energy. Calorimetry Study of heat absorbed or evolved in chemical reactions Calorimeter Device used in Calorimetry to measure heat processes (normally thermally insulated from the surroundings) Heat Capacity Thermochemistry – CHEM 1050. conditions of a system (temperature, pressure, composition) the total energy possessed by a system. the study of energy changes that occur during chemical reactions and changes in state. 0 o C expands from 3. At atmospheric pressure, helium can exist in all three phases, as well as a supercritical fluid phase near absolute zero. 42a Previous Answer Chapter 5 - Thermochemistry - Exercises - Page 205: 5. Adiabatic Work and EnergY. First Law of Thermodynamics. Need Help? delta Hf degrees; the change in enthalpy for the reaction that forms one mole of the substance from its elements in their most stable form with all reactants and products at 1atm pressure and usually 298 K; for any element at in its most stable state at 298 K and 1atm, delta Hf degrees=0 heat. Work. 2 days ago · 1 / 24. 5: Energy Basics Thermochemistry : the area of science concerned with the amount of heat absorbed or released during chemical and physical changes Energy o Energy : the capacity to supply heat or do work Potential Energy (PE) – the energy an object has because of its positon, composition, or condition Kinetic Energy (KE) – the energy that an object possesses Mar 20, 2019 · Chapter 5 - Thermochemistry Heat changes in chemical reactions. maycee____M. The measure of heat changes for physical and chemical processes. must be added. Chapter 5 - Thermochemistry. the study of energy transformations that occur in a collection of matter. a part of thermodynamics that involves the relationship between chemical rxns and heat changes. system. 64 L by increasing its temperature to 58. Learn about the AP Chemistry essentials. 39 terms. Temperature measures the average kinetic energy of molecules. Exercise 135c. Heat of Combustion. Flashcards. 5 ° C, and the temperature of the solution after mixing was 20. Chapter 19. Next Answer Chapter 5 - Thermochemistry - Exercises - Page 206: 5. If a reaction is exothermic the heats of formation of the products is _____ the heats of formation of the reactants. for doing work or. 52 terms. CuO(s) + H2(g) → Cu(s) + H2O(l) ΔH °. 2) bonds are broken and particles rearrange. Gasoline contains a significant amount of chemical potential energy. cp= Q/ (m) (𝚫T) Equation to find specific heat. Q= (cp) (m) (𝚫T) Equation to find heat energy. (The molar enthalpy of formation, ∆ , for H2O( ) is -285. docx. A balloon filled with 8. Less than. Less attraction (higher Eel) SI Unit of energy is the. Honors Lecture Notes: Unit 4. The thermochemical equation for the synthesis of water if ∆H is 285 kJ/mol. 0: Prelude to Thermochemistry. 0 g/cm 3 (1 g/mL) and that it takes as much energy to keep the water at 85 °F as to heat it from 72 °F to 85 °F. Exercise 136a. thermochemistry ↔ the study of heat absorbed or evolved by chemical reactions energy ↔ the potential or capacity to move matter. 3] — attraction/repulsion. Chem 5. temperature. Exothermic. AP Chemistry. Convert this energy to (a) kilojoules In thermochemistry, the state of the substances in the system must be shown: See Table 2 & Figure 7 on page 304 for more details of the above changes Molar Enthalpies: (5. Figure 5. 5. (a) 0. kj ww hr uy gm rf rc wi dq qb