Ch 11 Section 3 Flashcards

1
Q

joseph gay-lussac observed that 2 L of hydrogen can react with 1 L of oxygen to form 2 L of water vapor at

A

constant temperature and pressure

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2
Q

Lussac’s reaction shows a simple and definite 2:1:2 relationship between the volumes of the

A

reactants and the product

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3
Q

two volumes of hydrogen react with 1 volume of oxygen to produce 2 volumes of

A

water vapor

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4
Q

the 2:1:2 relationship for this reaction applies to any

A

proportions for volume

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5
Q

gay-lussac also noticed simple and definite proportions by

A

volume in other reactions of gases

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6
Q

Gay-Lussac’s law of combining volumes of gases states that at constant temperature and pressure, the volumes of gaseous reactnats and products can be expressed as

A

ratios of small whole numbers

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7
Q

law of combining volumes of gases as well as avogadro’s insight provided a better understanding of how gases react and

A

combine with each other

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8
Q

in 1811, avogadro found a way to explain Gay-Lussac’s simple ratios o combining volumes without violating Dalton’s idea of

A

indivisible atoms

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9
Q

avogadro rejected dalton’s idea that reactant elements are always in monatomic form when they

A

combine to form products

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10
Q

avogadro’s law states that equal volumes of gases at the same temperature and pressure contain

A

equal numbers of molecules

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11
Q

avogadro reasoned that molecules combining to form products could contain more than one

A

atom

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12
Q

at the same temperature and pressure, the volume of any given gas varies directly with the number of

A

molecules

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13
Q

avogadro’s law indicates that gas volume is directly proportional to the amount of

A

gas, at a given temp and pressure

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14
Q

V=

A

kn

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15
Q

avogadro’s reasoning applies to the combining volumes for the reaction of hydrogen and oxygen to form

A

water vvapor

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16
Q

while dalton thought the formula of water was HO, avogadro’s reasoning established that the formula must be

A

h2o

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17
Q

the coefficients in a chemical reaction involving gases indicate the relative numbers of …, the relative numbers of …, and the relative

A

molecules; moles; volumes

18
Q

experiments eventually showed that all elements that are gases near room temp, except noble gases, normally exist as

A

diatomic molecules

19
Q

according to avogadro’s law, one mole of any gas will occupy the same volume as one mole of any other gas at the same

A

temperature and pressure, despite mass differences

20
Q

the volume occupied by one mole of a gas at STP is known as the

A

standard molar volume of a gas and is 22.4 L

21
Q

knowing the volume of a gas, you can use 1 mol/ 22.4 L as a conversion factor to find the

A

number of moles, and mass, of a given volume of a given gas at STP

22
Q

you can use the molar volume of a gas to find the volume, at STP, of a known number of

A

moles or a known mass of a gas

23
Q

for gaseous reactants or products, coefficients in chemical equations not only indicate molar amounts and mole ratios but also reveal

A

volume ratios, assuming conditions remain the same

24
Q

the ideal gas law is the mathematical relationship among

A

pressure, volume, temperature, and the number of moles of a gas

25
Q

ideal gas law: PV=

A

nRT

26
Q

ideal gas law reduces to boyles’s law, charles’s law, gay-lussac’s law, or avogadro’s law when the appropriate variables are

A

held constant

27
Q

the number of molecules or moles present will always affect at least one of the other

A

three quantities

28
Q

the collision rate of molecules per unit area of container wall depends on the number of

A

molecules present

29
Q

if the number of molecules is increased for a sample at constant volume and temperature, the

A

collision rate increases and so does pressure

30
Q

according to avogadro’s law, if pressure and temp were kept constant while number of molecules increased, the

A

volume would increase

31
Q

an increase in volume keeps the pressure

A

constant at constant temperature

32
Q

increasing volume keeps the collision rate per unit of wall area

A

constant

33
Q

the constant R is known as the

A

ideal gas constant

34
Q

the value of r depends on the units chosen for

A

pressure, volume, and temperature

35
Q

measured values of P, V, T, and n for a gas at near-ideal conditions can be used to calculate

A

R

36
Q

R is used in calculations when volume is in … and temp is in

A

liters; kelvins

37
Q

ideal gas law can be applied to determine existing conditions of a gas sample when 3 of the 4 variables P,V, T, or n are

A

known

38
Q

ideal gas law can also be used to calculate the

A

molar mass or density of a gas sample

39
Q

for mm hg, r is

A

62.4

40
Q

for atm, r is

A

.082

41
Q

for J and kPa, R is

A

8.314