Chem 103 Module 6 Module 6 Portage Learning Chemistry Latest Updated 2024-2025 Actual Exam Questions and 100% Verified Correct Answers Guaranteed A+
bomb calorimeter - CORRECT ANSWER: device designed to measure the energy
change for processes occurring under conditions of constant volume; commonly used for reactions involving solid and gaseous reactants or products
calorie (cal) - CORRECT ANSWER: unit of heat or other energy; the amount of energy required to raise 1 gram of water by 1 degree Celsius; 1 cal is defined as 4.184 J
calorimeter - CORRECT ANSWER: a device used to measure the amount of heat
absorbed or released during chemical or physical processes
calorimetry - CORRECT ANSWER: process of measuring the amount of heat involved
in a chemical or physical process
chemical thermodynamics - CORRECT ANSWER: area of science that deals with the
relationships between heat, work, and all forms of energy associated with chemical and physical processes
endothermic process - CORRECT ANSWER: chemical reaction or physical change that
absorbs heat
energy - CORRECT ANSWER: the capacity to supply heat or do work
enthalpy (H) - CORRECT ANSWER: is an energy like internal energy (E). The most
important attribute of H is ΔH = Qp, the heat transferred at constant pressure
exothermic process - CORRECT ANSWER: chemical reaction or physical change that
releases heat
expansion work (pressure-volume work) - CORRECT ANSWER: work done as a
system expands or contracts against external pressure
first law of thermodynamics - CORRECT ANSWER: internal energy of a system
changes due to heat flow in or out of the system or work done on or by the system
heat (q) - CORRECT ANSWER: transfer of thermal energy between two substances
heat capacity (C) - CORRECT ANSWER: extensive property of a body of matter that
represents the quantity of heat required to increase its temperature by 1 degree Celsius (or 1 kelvin) 1 / 2
internal energy (E) - CORRECT ANSWER: sum of all kinetic and potential energies of the molecules in the system. It is the change in E that is useful to understand, and it is expressed through the first law of thermodynamics, ΔE = q + w.
joule (J) - CORRECT ANSWER: SI unit of energy; 1 joule is the kinetic energy of an object with a mass of 2kg moving with a velocity of 1 m/s, 1 J = 1 kg m2/s and 4.184 J =
- cal
kinetic energy - CORRECT ANSWER: energy of a moving body, in joules, equal to
1/2mv^2
potential energy - CORRECT ANSWER: energy of a particle or system of particles
derived from relative position, composition, or condition
specific heat capacity (c) - CORRECT ANSWER: intensive property of a substance that represents the quantity of heat required to raise the temperature of 1 gram of the substance by 1 degree Celsius (or 1 kelvin)
surroundings - CORRECT ANSWER: all matter other than the system being studied
system - CORRECT ANSWER: portion of matter undergoing a chemical or physical
change being studied
temperature - CORRECT ANSWER: intensive property of matter that is a quantitative measure of "hotness" and "coldness"
thermal energy - CORRECT ANSWER: kinetic energy associated with the random
movement of atoms or molecules
thermochemistry - CORRECT ANSWER: study of measuring the amount of heat
absorbed or released during a chemical reaction or a physical change
When 50.0 mL of 0.10 M HCl(aq) and 50.0 mL of 0.10 M NaOH(aq), both at 22.0 °C, are added to a coffee cup calorimeter, the temperature of the mixture reaches a maximum of 28.9 °C degrees. Would the amount of heat measured for this reaction be greater, lesser, or remain the same if we used a calorimeter that was a poorer insulator
than a coffee cup calorimeter? Explain your answer - CORRECT ANSWER: Lesser;
more heat would be lost to the coffee cup and the environment and so ΔT for the water would be lesser and the calculated q would be lesser
When solid ammonium nitrate dissolves in water, the solution becomes cold. This is the basis for an "instant ice pack". When 3.21 g of solid NH4NO3 dissolves in 50.0 g of water at 24.9 °C in a calorimeter, the temperature decreases to 20.3 °C. Would the amount of heat absorbed by the dissolution appear greater, lesser, or remain the same if the experimenter used a calorimeter that was a poorer insulator than a coffee cup
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