Thermochemistry (Test 3)
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| thermodynamics | the study of energy and its transformations
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| thermochemistry | the study of the relationship between chemical reactions and energy
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| energy | the capacity to do work
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| heat | the flow of energy caused by a temperature difference
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| work | the result of a force acting through a distance
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| What is the equation for work involving force and distance? | w = F times d
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| What is the equation for work involving pressure and volume? | w = - P (delta V)
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| kinetic energy | the energy associated with the motion of an object
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| What is the equation for kinetic energy? | Ek = (1/2)(m)(V^2)
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| potential energy | stored energy; energy due to position or composition (examples: chemical energy)
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| thermal energy | energy associated with the temperature of a substance
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| chemical energy | energy associated with the relative positions of electrons and nuclei in atoms and molecules
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| system | the part of the universe being studied
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| surroundings | everything else in the universe
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| internal energy of the system (E) | the sum total of all of the kinetic and potential energies of every particle in the system; unknowable
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| state function | a function that is independent of the history or path followed
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| What are some examples of state functions? | temperature, volume of a gas, location, molarity, internal energy, enthalpy, and change in any of these.
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| What is one joule equal to? | 1 (kg * m^(2))/(s^(2))
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| What is the First Law of Thermodynamics? | the law of conservation of energy; the total energy of the universe is constant.
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| What is the equation that expresses the First Law of Thermodynamics? | delta E = q + w, where delta E is the change in internal energy, q is heat, and w is work.
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| How do you determine if the sign of q is positive or negative? | q is positive if heat flows from the surroundings to the system; q is negative if heat flows from the system to the surroundings.
w is positive if the surroundings do work on the system; w is negative if the system does work on the surroundings.
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| calorimetry | measuring heat flow
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| calorimeter | an instrument used for measuring heat flow
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| bomb calorimeter | a constant volume calorimeter
delta E = q sub v, where q sub v is heat flow under constant volume
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| coffee-cup calorimeter | a constant pressure calorimeter
delta H = q sub p, where q sub p is heat flow under constant pressure
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| heat capacity | the amount of heat required to raise the temperature of a substance by 1 degree Celsius
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| specific heat capacity | the amount of heat required to raise the temperature of 1 g of a substance by 1 degree Celsius
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| What is the equation for heat? | q =(m)(c)(delta T)
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| When a problem involves two substances, how do you determine heat? | -q = q
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| In a bomb calorimeter (constant volume), what equation is used? | delta E = q sub v
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| How many joules are equal to 1 liter*atmosphere? | 101.3 J = 1 L*atm
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| delta H | enthalpy change; heat flow under constant pressure
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| An endothermic reaction has which sign of delta H? | positive
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| An exothermic reaction has which sign of delta H? | negative
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| The stoichiometric coefficients in a thermochemical reaction refer to what? | the number of moles of reactants and products
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| A reversed reaction has what effect on the delta H of that reaction? | changes the sign
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| The enthalpy change, delta H, is for what? | the specified number of moles
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| What is Hess's Law? | the total enthalpy change (delta H) for a process is the same regardless of whether the process occurs in one step or many steps
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| What is a formation reaction? | forming one mole of a substance from its elements in their most stable forms
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| Any element in its most stable form has what enthalpy of formation? | 0
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| To find delta H of a reaction using delta H of formations, always do what? | delta H formation of products - delta H formation of reactants
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