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57 Cards in this Set
- Front
- Back
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thermochemistry
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branch of thermodynamics that deals with the heat involved with chemical and physical changes
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energy
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potential to do work or transfer heat
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internal energy
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total energy of a system. (potential and kenetic)
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∆E
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E(final)-E(initial)
q(heat)+w(work) |
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1st law of thermodynamics
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energy of a system is constant (system+surroundings)
any energy transferred from a system must be transferred to the surroundings (and vice versa) |
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when ∆E is negative.....
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the reaction is exothermic.
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when ∆E is positive...
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the reaction is endothermic
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endothermic
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absorbs heat from the surroundings. (feels cold)
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exothermic
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transfers heat to the surroundings (feels hot)
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w (work) equals....
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-P∆V
P(external Pressure) V(volume) |
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in the work equation, if the equation ends with a negative number....
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work is being done on its surroundings
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in the work equation, if the equation ends with a positive number...
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work is being done on the system.
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∆ means...
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final-initial
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a combustion reaction is always endothermic or exothermic?
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exothermic
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∆H is....
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q (heat)
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H means what?
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enthalpy
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SI unit for a Joule
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1 kgm2/s2
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when enthalpy is negative is it exothermic or endothermic?
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it's exothermic
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when enthalpy i positive, is it exothermic or endothermic?
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it's endothermic
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enthalpy
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the sum of the internal energy of the system and the product of pressure and volume
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∆H (enthalpy change) of a reaction is
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the heat evolved in a reaction at constant pressure..
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if a thermometer goes up in temperature, is exothermic or endothermic?
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exothermic
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if a thermometer goes down in temperature, it's exothermic or endothermic?
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endothermic
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specific heat of water
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4.184 J/g*K
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q(reaction)= -q(solution) = -(mass * C * ∆T)
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reactions done in aqueous solution are at constant pressure in ∆H
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calorimetry (constant pressure calorimetry)
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-c*m*∆T
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specific heat definition
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amount of energy needed to raise 1 g of something by 1 degree.
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when there is a constant ∆V (∆V=0), then ∆H=q=∆E.
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q(cal)=C(cal) * ∆T
C(cal) is specific heat of calorimeter |
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enthalpy is what kind of property?
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extensive property.
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state functions
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depends only on the initial and final states of system, not on how the internal energy is used.
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standard state
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state of a material at a defined set of conditions.
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standard enthalpy change ∆H⁰
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is the enthalpy change when all reactants and products are in their standard states
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standard enthalpy of formation ∆H(f)⁰
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enthalpy change for reaction forming 1 mole of a pure compound from its constituent elements.
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Hess's Law
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if a reaction is carried out in a number of steps, ∆H for the overall reaction is the sum of ∆H for each individual step.
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1 atm is how many millibars?
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1 atm= 1013.25 millibars
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pressure and volume are directly or inversely proportional?
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inversely
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volume and temperature are directly or inversely proportional?
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directly
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if pressure goes up what happens to volume?
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volume goes down
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if volume goes up what happens to pressure?
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pressure goes down
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if temperature goes up what happens to volume?
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volume goes up
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if volume goes down what happens to temperature?
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temperature goes down
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miscible
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mix 1 gas with another to form a homogeneous solution
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pressure
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force acting on an object per unit area.
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atmospheric pressure
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the air is made up of gasses; those gasses are being acted upon by gravity and being pushed toward earth
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1 Pa = 1 N/m2
what's the units for N? |
kg*m/s2
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ideal gas equation
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PV=nRT
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what is the number for R?
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.08206 atm*L/mol*K
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1 mol is how many liters?
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1 mole = 22.4 L
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molar mass equation
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d*RT/P
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the density of a gas is ______ proportional to its molar mass
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directly
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the density of a gas is ______ proportional to the temperature
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inversely
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Boyle's Law
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states that the volume of a gas is inversely proportional to the pressure.
decreasing the volume forces the molecules into a smaller space. more molecules will collide with the container at any one instant, increasing the pressure |
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Charles's Law
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states the volume of a gas is directly proportional to the absolute temperature.
increasing the temp increases their avg speed, causing them to hit the wall harder and more frequently. in order to keep pressure constant, the volume must increase |
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Avogadro's Law
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states that the volume of a gas is directly proportional to the # of gas molecules.
increasing the # of gas molecules causes more of them to hit that wall at the same time. in order to keep pressure constant, the volume must then increase. |
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rate of effusion equation
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square root of M1/M2
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proportions of effusion rates
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the rate of effusion of a gas is inversely related to the square root of its molar mass.
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Van der Waals equation
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(P+n^2a/V^2)(v-nb) = nRT
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