Module 12 Flashcards

1
Q

State Charlie’s Law

A

under conditions of constant pressure, the temperature and volume are linearly proportional to each other
TEMP AND VOLUME PROPORTIONAL

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2
Q

Define boiling point

A

the temperature at which the liquid’s vapor pressure is equal to atmospheric pressure.
VAPOR PRESSURE EQUAL TO ATMOSPHERIC PRESSURE

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3
Q

pressure

A

the force per unit area exerted on an object P= F/A

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4
Q

Pascal (Pa)

A

the pressure unit of Newtons/ square m

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5
Q

1.000 atm =

A
  1. 3 kPa
  2. 0 torr
  3. 0 mmHg
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6
Q

Boyle’s Law

A

as long as the temperature of a gas stays the same, the product of the gas’ volume and its pressure is always the same PV= constant
GAS VOLUME AND PRESSURE IS SAME WITH A CONSTANT TEMP

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7
Q

Absolute temp scale

A

kelvin temp scale that can never reach 0 degrees

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8
Q

Extrapolation

A

following an established trend in the data even though there is no data available for that region

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9
Q

combined gas law

A

PV/ T = constant (p- pressure, v-volume, t- temp)

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10
Q

When using any equation in this module, I must always use

A

the Kelvin Temp scale

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11
Q

Ideal gas

A

a gas that applies to the combination gas law

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12
Q

three properties of an ideal gas

A

molecules/atoms that make it up are very small compared to the total volume available to the gas
MOLECULES SMALL COMPARED TO TOTAL VOLUME

molecules/atoms that make it up are so far apart from one another that there is no attraction or repulsion between them
MOLECULES WITH NO ATTRACTION/REPULSION

the collisions that occur between the gas molecules/atoms must be ELASTIC COLLISIONS

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13
Q

elastic in terms of this module

A

when molecules/ atoms collide with each other or the walls of the container, no energy is lost

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14
Q

Standard temp and Pressure (STP)

A

a temp of 273 K and a pressure of 1.00 atm

used as a reference to determine whether or not a gas is ideal

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15
Q

A gas with a temp that is … and a pressure that is… will behave in an ideal fashion.

A
close to (or larger than) 273 K
near (or lower than) 1.00 atm
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16
Q

Daltons law of Partial Pressures

A

when ideal gases are mixed, the total pressure of the mixture is equal to the sum of the pressures of each individual gas Pt = P1 + P2 + P3 + …

(Pt= total pressure) (P1, P2 etc are referred to as PARTIAL PRESSURES)

17
Q

The pressure of an ideal gas does not depend on the … It depends only on the…

A

identity of the gas

quantity of that gas

18
Q

vapor pressure

A

the pressure exerted by the vapor which sits on top of any liquid

19
Q

the vapor pressure of any liquid …

A

increases with increasing temp

20
Q

mole fraction

A

X = # of moles of component/ total # of moles in the mixture