EN CHEM 1 - CHEMISTRY FOR ENGINEERS PDF

Republic of the Philippines CAMARINES NORTE STATE COLLEGE F. Pimentel Avenue, Brgy....

Republic of the Philippines CAMARINES NORTE STATE COLLEGE F. Pimentel Avenue, Brgy. 2, Daet, Camarines Norte – 4600, Philippines COLLEGE OF ENGINEERING EN CHEM 1 – CHEMISTRY FOR ENGINEERS Subject Instructor: Engr. Yves Djonly M. Villagracia Module No. & Title: 2. Energy and Chemistry ================================================================================= 2. Energy and Chemistry Y Outline of Topics L 1. Nature of Energy N 2. Forms of Energy 3. Conversion of Energy O 4. Law of Conservation of Energy 5. Thermochemistry S 6. Endothermic Reaction 7. Exothermic Reaction E 8. Specific Heat S Specific Intended Learning Outcome/s (SILOs) O At the end of this topic, the student should be able to:  Understand the relationship of chemistry and energy P  Classify the different forms of energy  Explain the energy conversion  State the law of conservation of energy R U  Know the principles of thermochemistry P  Differentiate Exothermic reaction from Endothermic reaction  Define and apply the principle of specific heat ================================================================================= N O Lesson 1: Nature of Energy IT Modern civilization is possible because people have learned how to change energy from one form to C another and then use it to do work. People use energy to walk and bicycle, to move cars along roads and boats through water, to cook food on stoves, to make ice in freezers, to light our homes and offices, to manufacture U products, and to send astronauts into space. Scientists define energy as the ability to do work. R Energy is essential to life and all living organisms. Our energy choices and decisions impact Earth's natural systems in ways we may not be aware of, so it is essential that we choose our energy sources T carefully. The true cost of energy is more than just dollars and cents; there are important economic, S political and social factors and consequences to consider as well. N It may exist in potential, kinetic, thermal, electrical, chemical, nuclear, or other various forms. Energy can be transferred in one of two ways – as heat, or as work, energy in the process of transfer from one I body to another. After it has been transferred, energy is always designated according to its nature. Heat is R the term given to energy that is transferred from a hot object to a cooler object due to the difference in their temperatures. Hence, heat transferred may become thermal energy, while work is the term given to energy O that is transferred as a result of a force applied over a distance, work done may manifest itself in the form F of mechanical energy. The energy we use to power everything from our homes to schools and workplaces comes from a variety of different sources. These can be broken down into renewable and non-renewable energy sources. EN CHEM 1 – Chemistry for Engineers Page 1 of 1  Republic of the Philippines CAMARINES NORTE STATE COLLEGE F. Pimentel Avenue, Brgy. 2, Daet, Camarines Norte – 4600, Philippines COLLEGE OF ENGINEERING 2 -2 Unit of Energy SI Unit: Joule (J) 1 J = 1 kgm s 1 calories = 4.184 Joules 1 BTU(British Thermal Unit) =252 calories 1 kWh = 3600 kJ = 3413 BTU = 860 kcal 7 1 Joule = 1×10 ergs YL Lesson 2: Forms of Energy N O Energy exists in many different forms, but they all fall into two basic categories Potential energy and Kinetic energy. S  Potential energy is any form of energy that has stored potential that can be put to future use. E PE = mgh WHERE: m – mass, g – acceleration due to gravity, h – altitude/height S  Chemical energy is energy stored in the bonds of atoms and molecules. Batteries, biomass, O petroleum, natural gas, and coal are examples of chemical energy. P  Nuclear energy is energy stored in the nucleus of an atom—the energy that holds the nucleus together. Large amounts of energy can be released when the nuclei are combined examples of nuclear energy. R (fusion) or split (fission) apart. Nuclear fission, nuclear fusion, and nuclear decay are UP  Kinetic energy is the motion of waves, electrons, atoms, molecules, substances, and objects. 1 2 KE = mv WHERE: m – mass, v ¬– velocity of object N 2 O  Radiant energy is electromagnetic energy that travels in transverse waves. Radiant energy includes visible light, x-rays, gamma rays, and radio waves. Light is one type of radiant IT energy. C  Thermal energy, or heat, is the energy that comes from the movement of atoms and molecules in a substance. Heat increases when these particles move faster. Geothermal U energy is the thermal energy in the earth. R  Mechanical energy is the energy a substance or system has because of its motion like T machines use mechanical energy to do work. Another examples are rolling bicycle, moving S gears, and running cars. N  Electrical energy is delivered by tiny charged particles called electrons, typically moving through a wire. Lightning is an example of electrical energy in nature. Other forms of energy I are also converted to electrical energy. For example, power plants convert chemical energy R stored in fuels like coal into electricity through various changes in its form. O  Sound Energy is produced when an object is made to vibrate. Sound energy travels out as F waves in all directions. Sound needs a medium to travel through, such as air, water, wood, and even metal. Examples of sound energy are voices, whistles, horns and musical instruments EN CHEM 1 – Chemistry for Engineers Page 2 of 2  Republic of the Philippines CAMARINES NORTE STATE COLLEGE F. Pimentel Avenue, Brgy. 2, Daet, Camarines Norte – 4600, Philippines COLLEGE OF ENGINEERING Lesson 3: Conversion of Energy Energy conversion, the transformation of energy from forms provided by nature to forms that can be used by humans. The same amount of energy exists after the conversion as before. Energy conversion obeys the law of conservation of energy. Y Energy can be converted from one form to another. For example, the food a person eats contains L chemical energy, and a person's body stores this energy until he or she uses it as kinetic energy during N work or play. The stored chemical energy in coal or natural gas and the kinetic energy of water flowing in rivers can be converted to electrical energy, which in turn can be converted to light and heat. O Over the centuries a wide array of devices and systems has been developed for this purpose. Some of these energy converters are quite simple. The early windmills, for example, transformed the kinetic S energy of wind into mechanical energy for pumping water and grinding grain. E Other energy-conversion systems are decidedly more complex, particularly those that take raw energy from fossil fuels and nuclear fuels to generate electrical power. Systems of this kind require S multiple steps or processes in which energy undergoes a whole series of transformations through various O intermediate forms. P The energy we use to power everything from our homes to schools and workplaces comes from a variety of different sources. These can be broken down into renewable (wind energy, solar energy, hydropower and geothermal energy) and non-renewable energy (oil, coal and natural gas) sources.R U Renewable energy is any natural energy resource that can replace itself quickly and dependably. P Non-renewable energy is a source of energy that will eventually run out. Most are fossil fuels. N Many transformations of energy are of practical importance. Combustion of fuels results in the conversion of chemical energy into heat and light. In the electric storage battery chemical energy is O converted to electrical energy and conversely. In the photosynthesis of starch, green plants convert light energy from the sun into chemical energy. Hydroelectric facilities convert the kinetic energy of falling water IT into electrical energy, which can be conveniently carried by wires to its place of use. C U Lesson 4: Law of Conservation of Energy R It is common for energy to be converted from one form to another; however, the law of T conservation of energy, a fundamental law of physics, states that although energy can be changed in form it can be neither created nor destroyed, the energy of the universe is constant. Another way of stating this S law of chemistry is to say the total energy of an isolated system remains constant or is conserved within a N given frame of reference. I If a stick of dynamite explodes, for example, the chemical energy contained within the dynamite R changes into kinetic energy, heat, and light. If all this energy is added together, it will equal the starting chemical energy value. O The conservation of energy in a physical system can be F illustrated by changes in the mechanical energy of a falling object. Mechanical energy consists of two types of energy: potential, or stored energy, and kinetic energy, the energy of motion. EN CHEM 1 – Chemistry for Engineers Page 3 of 3 SOURCE: https://kids.britannica.com/students/article/conservation-of- /570822  Republic of the Philippines CAMARINES NORTE STATE COLLEGE F. Pimentel Avenue, Brgy. 2, Daet, Camarines Norte – 4600, Philippines COLLEGE OF ENGINEERING For example, all of the mechanical energy in a boulder at rest on a hilltop is potential energy. When the boulder falls, some of its potential energy changes into kinetic energy. The faster the boulder moves, the greater its kinetic energy and the less its potential energy. As the boulder slows, the amount of kinetic energy decreases and the amount of potential energy increases. When the boulder stops moving at the bottom of the hill, all of the kinetic energy it contained will have changed into potential energy. Y This can be expressed as follows: L initial potential energy + initial kinetic energy = final potential energy + final kinetic energy N The law of conservation of energy also applies to other O forms of energy. When a lamp is turned on, some of the electrical energy in the lamp is converted to light energy, though S most may be changed to thermal energy, or heat. The total amount of energy in the system before the lamp was switched E on will equal the total energy afterward, even though the form of S energy changed. O P This can be expressed as follows: SOURCE: https://kids.britannica.com/students/article/conservation-of- /570822 R electrical energy = light energy + thermal energy UP For example, if the lamp contained 200 joules (J) of electrical energy at the beginning, and 20 J were converted to light energy, then the amount of electrical energy converted to thermal energy would be 180 J: N 200 J (electrical energy) → 20 J (light energy) + 180 J (thermal energy) O IT In a chemical system, energy is contained within chemical bonds. Energy is released when bonds are formed between molecules in a chemical reaction; when molecules are broken down, the energy is released. As with physical systems, however, the total amount of energy at the start of a chemical C reaction must equal the total amount at the end. U R Lesson 5: Thermochemistry T Thermochemistry is the study of the heat released or absorbed as a result of chemical reactions. It S is a branch of thermodynamics and is utilized by a wide range of scientists and engineers. For example, N biochemists use thermochemistry to understand bioenergetics, whereas chemical engineers apply thermochemistry to design manufacturing plants. Chemical reactions involve the conversion of a set of I substances collectively referred to as "reactants" to a set of substances collectively referred to as "products." R O Thermochemical changes are often discussed in terms of the "system" and the "surroundings." The system is regarded as the reaction products and reactants, whereas the surroundings consist of everything F else in the universe. A boundary separates the system from the surroundings. EN CHEM 1 – Chemistry for Engineers Page 4 of 4  Republic of the Philippines CAMARINES NORTE STATE COLLEGE F. Pimentel Avenue, Brgy. 2, Daet, Camarines Norte – 4600, Philippines COLLEGE OF ENGINEERING A system is the specific portion of the universe that is being studied. Everything outside the system is considered the surroundings or environment. A system may be: Y  A Isolated System which can L exchange neither energy nor matter with the surroundings, such as an insulated bomb N calorimeter  A Closed System which can O exchange energy but not matter, such as an uninsulated closed piston or balloon S  An Open System which it can E SOURCE: https://www.slideshare.net/CtMutiahMazait/80-thermochemistry-students-copy?qid=f4a9f1fe-927f exchange both matter and energy with the -4854-b52e-053858ac9513&v=&b=&from_search=26 surrounding, such as a pot of boiling water S O Two fundamental principles of thermochemistry are: 1. Lavoisier and Laplace’s law (1780): The energy change in any transformation is equal and P opposite to energy change in the reverse process. 2. Hess' law (1840): The energy change in any transformation is the same whether the process occurs in one step or many. R U These statement helps in formulation of first law of thermodynamics in 1845. Lavoisier, P Laplace and Hess also investigated specific heat and latent heat, although it was Joseph Black who made the most important contributions to the development of latent energy changes. N The study of energy and its interconversions is called thermodynamics. The law of conservation of O energy is often called the first law of thermodynamics and is stated as follows: The energy of the universe is constant. IT Calorimetry The device used experimentally to determine the heat C associated with a chemical reaction is called a calorimeter. Calorimetry, the science of measuring heat, is based on observing the temperature change when U a body absorbs or discharges energy as heat. R The measurement of heat using a simple calorimeter such as that T shown in Figure, (is a coffee cup calorimeter made of two Styrofoam cups), is an example of constant-pressure calorimetry, since the pressure (atmospheric S pressure) remains constant during the process. Constant-pressure calorimetry is used in determining the changes in enthalpy (heats of reactions) for reactions N occurring in solution. I The heat capacity of the entire calorimeter may be obtained by measuring the change in temperature of the surroundings resulting from a R known heat input. O Known amount of heat = calorimeter constant × ∆T F SOURCE: Chemistry Second Edition by Zumdahl and or Zumdahl q = Ccalorimeter × ∆T There is no mass or number of moles term here for the quantity of material. The calorimeter EN CHEM 1 – Chemistry for Engineers Page 5 of 5  Republic of the Philippines CAMARINES NORTE STATE COLLEGE F. Pimentel Avenue, Brgy. 2, Daet, Camarines Norte – 4600, Philippines COLLEGE OF ENGINEERING constant is the heat capacity of a particular object (or set of objects) rather than that of a material. Once the calorimeter constant is known, we are ready to use the calorimeter for our actual measurement. We place known amounts of reactant(s) into the calorimeter, initiate the reaction, and then measure the resulting temperature change of the calorimeter. The calorimeter constant allows us to determine the amount of heat released or absorbed in the reaction. Y Commonly includes calculations of: L 1. The Enthalpy is a state function. A change in enthalpy does not depend on the pathway between N two states. The enthalpy H,( H = E + PV, where E is the internal energy of the system, P is the pressure of the system, and V is the volume of the system). O ∆H = qp At constant pressure (where only PV work is allowed), the change in enthalpy H of the S system is equal to the energy flow as heat. This means that for a reaction studied at constant E pressure, the flow of heat is a measure of the change in enthalpy for the system. S For a chemical reaction, the enthalpy change is given by the equation ∆H = Hproduct - Hreactants O At constant pressure, exothermic means ΔH is negative; endothermic means ΔH is positive. P 2. The internal energy E of a system can be defined most precisely as the sum of the kinetic and changed by a flow of work, heat, or both. That is, R potential energies of all the “particles” in the system. The internal energy of a system can be U ∆E = q + w P Where ∆E represents the change in the system’s internal energy, q represents heat, and w N represents work. 3. The heat capacity C of a substance, which is a measure of this property, is defined as O heat absorbed C= IT increase in temperature C When an element or a compound is heated, the energy required will depend on the amount of the substance present. Thus, in defining the heat capacity of a substance, the amount of U substance must be specified. If the heat capacity is given per gram of substance, it is called the specific heat capacity, and its units are J/°Cg or J/Kg. If the heat capacity is given per mole of the R substance, it is called the molar heat capacity, and it has the units J/°C mol or J/K mol. TSN R I O F EN CHEM 1 – Chemistry for Engineers Page 6 of 6  Republic of the Philippines CAMARINES NORTE STATE COLLEGE F. Pimentel Avenue, Brgy. 2, Daet, Camarines Norte – 4600, Philippines COLLEGE OF ENGINEERING Lesson 6: Endothermic Reaction Endothermic reactions are reactions that require external energy, usually in the form of heat, for the reaction to proceed. Since endothermic reactions draw in heat from their surroundings, they tend to cause their environments to cool down. Y Example Reaction: LN 1) Photosynthesis: Plants absorb heat energy from sunlight to convert carbon dioxide and water into glucose and oxygen. O 6CO2 + 6 H2O + heat ---> C6H12O6 + 6O2 S 2) Cooking an egg: Heat energy is absorbed from the pan to cook the egg. E They are also generally non- S spontaneous, since endothermic reactions O yield products that are higher in energy than the reactants. As such, the change in enthalpy for P an endothermic reaction is always positive. In an endothermic reaction, the R U products (C in diagram) are higher in energy P than the reactants (A+B in diagram). Therefore, the change in enthalpy is positive, and heat is N absorbed from the surroundings by the reaction. O SOURCE: https://courses.lumenlearning.com/introchem/chapter/exothermic-and-endothermic- Whether a reaction is endothermic or IT exothermic depends on the direction that it is going; some reactions are reversible, and when you revert the products back to reactants, the change in C enthalpy is opposite. U R TSN R I O F EN CHEM 1 – Chemistry for Engineers Page 7 of 7  Republic of the Philippines CAMARINES NORTE STATE COLLEGE F. Pimentel Avenue, Brgy. 2, Daet, Camarines Norte – 4600, Philippines COLLEGE OF ENGINEERING Lesson 7: Exothermic Reaction Exothermic reactions are reactions or processes that release energy, usually in the form of heat or light. 1. Combustion: The burning of carbon-containing compounds uses oxygen, from air, and produces carbon dioxide, water, and lots of heat. For example, combustion of methane (CH4) can be Y represented as follows: LN CH4 + 2(O2) ---> CO2 + 2H2O + heat O 2. Rain: Condensation of water vapor into rain releasing energy in the form of heat is an example of an exothermic process. S In an exothermic reaction, energy is released because the total energy of the products is less than E the total energy of the reactants. For this reason, the change in enthalpy, for an exothermic reaction will always be negative. S O In an exothermic reaction, the total P energy of the products (C in diagram) is less than the total energy of the reactants (A+B in diagram). Therefore, the change in enthalpy is negative, and heat is released to the R U surroundings. P N O IT SOURCE: https://courses.lumenlearning.com/introchem/chapter/exothermic-and-endothermic- C U Endothermic vs Exothermic Comparison R Here's a quick summary of the differences between endothermic and exothermic reactions: T Endothermic Exothermic S heat is absorbed (feels cold) heat is released (feels warm) N energy must be added for reaction to occur reaction occurs spontaneously disorder decreases (ΔS < 0) entropy increases (ΔS > 0) I increase in enthalpy (+ΔH) decrease in enthalpy (-ΔH) R SOURCE: https://www.thoughtco.com/endothermic-and-exothermic-reactions-602105 O F EN CHEM 1 – Chemistry for Engineers Page 8 of 8  Republic of the Philippines CAMARINES NORTE STATE COLLEGE F. Pimentel Avenue, Brgy. 2, Daet, Camarines Norte – 4600, Philippines COLLEGE OF ENGINEERING Lesson 8: Specific Heat The specific heat is the amount of heat per unit mass required to raise the temperature by one degree Celsius. The relationship between heat and temperature change is usually expressed in the form shown below where c is the specific heat. Y specific heat capacity (c, usually L simply called the specific heat) N Q = cm∆T O Where: Q – Heat m - mass S C – specific heat E ∆T – Change in temperature S Molar heat capacity is a physical O property that describes how much heat is required to raise the temperature of one mole P of a substance by 1°C. So if we choose to express the amount of material in terms of moles rather than R U mass, our equation changes only slightly. P Q = nCp∆T N O Where: Q – Heat n – mole IT Cp – Heat capacity at constant pressure (Under other conditions, C SOURCE: Chemistry for Engineering Students Second Edition by Brown and Holme such as constant volume, the value of the heat capacity may differ slightly.) U ∆T – Change in temperature R TSN R I O F SOURCE: https://www.britannica.com/science/specific- EN CHEM 1 – Chemistry for Engineers Page 9 of 9  Republic of the Philippines CAMARINES NORTE STATE COLLEGE F. Pimentel Avenue, Brgy. 2, Daet, Camarines Norte – 4600, Philippines COLLEGE OF ENGINEERING References: Chemistry Second Edition by Zumdahl and Zumdahl Chemistry for Engineering Students Second Edition by Brown and Holme What is energy? explained. (2020, June 18). U.S. Energy Information Administration (EIA). Y https://www.eia.gov/energyexplained/what-is-energy/ LN Conservation of energy. (n.d.). Britannica Kids. https://kids.britannica.com/students/article/conservation-of- energy/570822 O Thermochemistry. (n.d.). Chemistry Explained. https://www.chemistryexplained.com/Te-Va/Thermochemistry.html S Exothermic and endothermic processes | Introduction to chemistry. (n.d.). Lumen Learning – Simple Book Production. https://courses.lumenlearning.com/introchem/chapter/exothermic-and-endothermic-processes/ ES Endothermic vs. exothermic reactions (article). (n.d.). Khan Academy. https://www.khanacademy.org/test- prep/mcat/chemical-processes/thermochemistry/a/endothermic-vs-exothermic-reactions O R P UP N O IT C U R TSN R I O F EN CHEM 1 – Chemistry for Engineers Page 10 of 10  Republic of the Philippines CAMARINES NORTE STATE COLLEGE F. Pimentel Avenue, Brgy. 2, Daet, Camarines Norte – 4600, Philippines COLLEGE OF ENGINEERING EN CHEM 1 – CHEMISTRY FOR ENGINEERS Period: ___________________ Name of Student: ____________________________________________Course and Year: __________ Schedule (Time and Day): _____________________________________Final Rating: ______________ ================================================================================= Direction: Accomplished and submit only the assessment task on the next delivery of learning materials. Y Assessment Task LN 1. Perform each of the following conversion. Show your solution and box your answer. a. 10,000 Joule to calories O S E 12 b. 1×10 ergs to Joules S O P c. 1 BTU to Joules R UP d. 360 Joules to cal N O 4 e. 16×10 calories to kcal IT C U 2. Give 5 examples of energy changing from one form to another. R TSN R I 3. Can you think of other fun examples of energy changing between kinetic and potential energy? O F EN CHEM 1 – Chemistry for Engineers Page 11 of 11  Republic of the Philippines CAMARINES NORTE STATE COLLEGE F. Pimentel Avenue, Brgy. 2, Daet, Camarines Norte – 4600, Philippines COLLEGE OF ENGINEERING 4. Classify each statement if the reaction occur is endothermic reaction or exothermic reaction. a. Mixing an acid and a base to form a salt and water __________________ b. Melting ice cubes __________________ c. Making an anhydrous salt from a hydrate __________________ d. Respiration __________________ e. Splitting a gas molecule __________________ Y f. Separating ion pairs __________________ L g. Corrosion of metal __________________ h. Evaporating liquid water __________________ N i. Most polymerization reactions __________________ j. Cooking an egg __________________ O k. Baking bread __________________ l. The thermite reaction __________________ S m. Combustion of a fuel __________________ n. Forming a cation from an atom in the gas phase __________________ E o. Nuclear fission __________________ S p. Converting frost to water vapor __________________ q. Dissolving an acid in water __________________ O r. Melting solid salts __________________ P 5. Determine if the equation is endothermic reaction or exothermic reaction a. CH4(g) + 2O2(g) → CO2(g)+ 2H2O(g) + energy (heat) b. Na(s) + 0.5Cl2(s) → NaCl(s) R U __________________ __________________ c. N2(g) + O2(g) + energy (heat) → 2NO(g) __________________ P d. sunlight + 6CO2(g) + H2O(l) → C6H12O6(aq) + 6O2(g) __________________ e. C6H12O6 + 6O2 → 6CO2 + 6H2O + Energy __________________ N 6. Calculate ΔE for a system undergoing an endothermic process in which 15.6 kJ of heat flows and where 1.4 kJ of work is done on the system. Show your solution and box your answer. O IT C U R T 7. A calorimeter is to be used to compare the energy content of some fuels. In the calibration of the S calorimeter, an electrical resistance heater supplies 100.0 J of heat and a temperature increase of 0.850°C is observed. Then 0.245 g of a particular fuel is burned in this same calorimeter, and the N temperature increases by 5.23°C. Calculate the energy density of this fuel, which is the amount of energy liberated per gram of fuel burned. Show your solution and box your answer. R I O F 8. When 1 mole of methane (CH4) is burned at constant pressure, 890 kJ of energy is released as heat. Calculate ΔH for a process in which a 5.8-g sample of methane is burned at constant pressure. EN CHEM 1 – Chemistry for Engineers Page 12 of 12  Republic of the Philippines CAMARINES NORTE STATE COLLEGE F. Pimentel Avenue, Brgy. 2, Daet, Camarines Norte – 4600, Philippines COLLEGE OF ENGINEERING Show your solution and box your answer YLN 9. Heating a 24.0-g aluminum can raises its temperature by 15.0°C. Find the value of q for the can. O Show your solution and box your answer S ES O R P U 10. The molar heat capacity of liquid water is 75.3 J/mol K. If 37.5 g of water is cooled from 42.0 to 7.0°C, what is q for the water? Show your solution and box your answer. P N O IT C U 11. Determine the heat needed to raise a 1 kg of iron from 250° C to 700° C? Note: Specific heat of iron, C = 0.45 J/g°C. Show your solution and box your answer. R TSN R I O F Conceptual Question Instructions: Analyze the scenario below and answer the following question. EN CHEM 1 – Chemistry for Engineers Page 13 of 13  Republic of the Philippines CAMARINES NORTE STATE COLLEGE F. Pimentel Avenue, Brgy. 2, Daet, Camarines Norte – 4600, Philippines COLLEGE OF ENGINEERING 1. Consider the following scenario. A car for which friction is not negligible accelerates from rest down a hill, running out of gasoline after a short distance. The driver lets the car coast farther down the hill, then up and over a small crest. He then coasts down that hill into a gas station, where he brakes to a stop and fills the tank with gasoline. Identify the forms of energy the car has, and how they are changed and transferred in this series of events. See Y Figure below. LN O S ES O R P UP N O IT C U R T 2. The brakes in a car increase in temperature by ΔT when bringing the car to rest from a S speed v. a. How much greater would ΔT be if the car initially had twice the speed? N R I O F b. You may assume the car stops fast enough that no heat transfers out of the brakes. EN CHEM 1 – Chemistry for Engineers Page 14 of 14  Republic of the Philippines CAMARINES NORTE STATE COLLEGE F. Pimentel Avenue, Brgy. 2, Daet, Camarines Norte – 4600, Philippines COLLEGE OF ENGINEERING YL 3. The same heat transfer into identical masses of different substances produces different temperature changes. Calculate the final temperature when 1.00 kcal of heat transfers into N 1.00 kg of the following, originally at 20.0°C: O a. water b. concrete c. steel S d. mercury ES O R P UP N O IT Student’s Corner C Write your feedback and learning in the lesson. U R TSN R I O F EN CHEM 1 – Chemistry for Engineers Page 15 of 15