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Pressure= 1.0 atm (or 760mmHg)
Temperature= 0*C |
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Boyle's Law:
If V increases, what does P do? |
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Charles's Law:
If T is lowered, V does what? |
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Charles's Law:
If T is raised, what happens to P? |
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Avogadro's Law:
If you remove gas, what happens to V? |
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| What is the proportionality constant? |
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R= PV/nT
R= 0.082057 (L*atm/K*mol) |
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| At STP, an ideal gas occupies what amount of Liters? |
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| Equation for calculating molar mass of a gaseous substance: |
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Definition
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| Root-mean-square (rms) speed (u rms) is: |
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| An average of molecular speed. |
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| The gradual mixing of molecules of one gas with molecules of another by virtue of their Kinetic properties is the definition of: |
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Definition
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| The process by which a gas under pressure escapes from one compartment of a container to another by passing through a small opening is the definition of: |
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| Boyle's equation for calculating pressure or volume changes |
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| Charles's equation for calculating temperature or volume changes: |
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| Charles's equation for calculating temperature or pressure changes: |
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| Combined gas equation for initial and final states: |
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Definition
| [(P1*V1)/(n1*T1)]=[(P2*V2)/(n2*T2)] |
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| Equation for calculating changes in pressure, temperature, or volume when mols is constant: |
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Definition
| [(P1*V1)/T1]=[(P2*V2)/T2] |
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| Equation for calculate the density of a gas: |
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| Dalton's Law of partial pressure calculation: |
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| Equation for root-mean-square speed of gas molecules: |
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Definition
| u rms= square root of(3RT/M) |
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| Grahm's Law of diffusion/effision equation: |
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Definition
| [(r1/r2)/square root of (M2/M1)] |
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| van der Waal's Equation for calculating pressure of a non ideal gas: |
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