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15 Cards in this Set
- Front
- Back
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define one mole |
one mole of any substance is the amount of that substance which contains the same number of particles as there are in 0.012kg of carbon 12 |
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what is boyle's law? |
the pressure of a fixed mass of gas is inversely proportional to it's volume given the temp is constant |
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what is the formula for charles's law? |
V1/T1= constant |
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what is the explanation to forces between particles are negligible, except during collisions. |
particles are attracted each other strongly over long distances, they would all tend to clump together in the middle in the container. The particles travel in straight lines between collisions |
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explanation for volume of the particles is negligible compared to volume occupied by the gas |
when a liquid boils to become a gas the particles become much further apart |
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explanation for collisions of particles with each other and with the container are perfectly elastic , no KE lost |
KE cannot be lost, total internal energy is the total KE of particles |
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what is the value of Boltzmann constant? |
R/ Na, k , is 1.38 x 10^-23 JK^-1 |
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formula for relationship of temp and molecular KE? and how to derive? |
pV=nRT and pV=1/3 Nm<c^2> nRT= 1/3 Nm<c^2> 1/2m<c^2>= 3/2 kT |
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how does KE relate to the thermodynamic temp? |
the mean translational Ke of an atom of an ideal gas is proportional to the thermodynamic temp. |
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In air there is a mixture of gases how does different gases move at same speed? ex.O2 and CO2 |
Co2 has greater mass than O2 so it moves slower. all the gases are colliding with one another and sharing energy. |
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pv=nRT but pv can also be equaled to what? |
pv=nKT |
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formula for square root of mean square speed? |
c^2 = 3/2 kT/m |
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how is the root mean square related to the absolute temp and mass? |
it is directly related to the square root of the absolute temp and inversely related to the square root of the mass m |
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what is internal energy of an ideal gas? |
the total internal energy is determined by the total KE because there are no intermolecular forces so there are no PE in an ideal gas |
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for chem, why do ideal gases not behave ideally in low temp and high pressure? |
at low temp, the forces between the molecules are important at high pressure, the volume of molecules is significant |
