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Gas Laws
- Stoichiometry
- Volume-Volume
- Problems Involving the volumes of both known and unknown quantities
- Problems Involving the volumes of both known and unknown quantities
- Mixed Mass-Volume-Mole-Particle
- Find the unknown at STP
- Then use 22.4mol=1L
- Find the unknown at STP
- Mass-Volume (Non-STP)
- Use the proportions in chemical equations
- Varied number of steps.
- Use the proportions in chemical equations
- Volume-Volume
- Combined Gas Laws
- P1V1/T1=P2V2/T2
- Charles' Law
- V1/T1=V2/T2
- Fixed pressure, temp/volume direct relationship
- V1/T1=V2/T2
- Boyle's Law
- P1V1=P2V2
- Fixed temp, volume/pressure inverse relationship.
- P1V1=P2V2
- Gay Lussac's Law
- P1/T1=P2/T2
- Fixed volume, temp/pressure direct relationship.
- P1/T1=P2/T2
- Combines Boyle's, Charles', and Gay Lussac's Laws.
- P1V1/T1=P2V2/T2
- Dalton's Law of Partial Pressures
- Total pressure of a mixture of gases is equal to the sum of the partial pressures of the component gasses
- Pt=P1+P2+P3....
- Partial Pressure over Water
- P(t)=P(g)+P(h2o)
- P(t)=P(g)+P(h2o)
- Total pressure of a mixture of gases is equal to the sum of the partial pressures of the component gasses
- Ideal Gas Law
- PV=nRT
- R=0.0821Latm/molK
- R=0.0821Latm/molK
- PV/nT=R
- R=8.31kPadm^3/molK
- R=8.31kPadm^3/molK
- For ideal gasses: PV/T and the number of moles is equal to a constant.
- PV=nRT
- Graham's Law of Diffusion
- Under the same conditions of T and P, gasses diffuse at rates that are inversely proportional to the
square root of their densities.
- D1/D2=(squrt)M1/M2
- Under the same conditions of T and P, gasses diffuse at rates that are inversely proportional to the
square root of their densities.
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