Examples of volume in the following topics:
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- Charles' Law describes the relationship between the volume and temperature of a gas.
- This law states that at constant pressure, the volume of a given mass of an ideal gas increases or decreases by the same factor as its temperature (in Kelvin); in other words, temperature and volume are directly proportional.
- A car tire filled with air has a volume of 100 L at 10°C.
- If a gas contracts by 1/273 of its volume for each degree of cooling, it should contract to zero volume at a temperature of –273°C; this is the lowest possible temperature in the universe, known as absolute zero.
- The lower a gas' pressure, the greater its volume (Boyle's Law), so at low pressures, the fraction \frac{V}{273} will have a larger value; therefore, the gas must "contract faster" to reach zero volume when its starting volume is larger.
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- Real gases deviate from the ideal gas law due to the finite volume occupied by individual gas particles.
- Ideal gases are assumed to be composed of point masses whose interactions are restricted to perfectly elastic collisions; in other words, a gas particles' volume is considered negligible compared to the container's total volume.
- At high pressures where the volume occupied by gas molecules does not approach zero
- The particles of a real gas do, in fact, occupy a finite, measurable volume.
- At high pressures, the deviation from ideal behavior occurs because the finite volume that the gas molecules occupy is significant compared to the total volume of the container.
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- Avogadro's Law states that at the same temperature and pressure, equal volumes of different gases contain an equal number of particles.
- V is the volume of the gas, n is the number of moles of the gas, and k is a proportionality constant.
- The barrier moves when the volume of gas expands or contracts.
- What is the relationship between the number of molecules and the volume of a gas?
- (Note: Although the atoms in this model are in a flat plane, volume is calculated using 0.1 nm as the depth of the container.)
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- The effects of changes in volume and pressure on a reversible reaction in chemical equilibrium can be predicted by Le Chatelier's Principle.
- The effects of changes in volume and pressure on chemical equilibrium can be predicted using Le Chatelier's Principle.
- This principle can be applied to changes in temperature, concentration, volume, and pressure.
- One example of the effect of changing volume is shown in .
- As can be seen, a reduction in volume yields an increase in the pressure of the system, because volume and pressure are inversely related.
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- Boyle's Law describes the inverse relationship between the pressure and volume of a fixed amount of gas at a constant temperature.
- In this case, the initial pressure is 20 atm (P1), the initial volume is 1 L (V1), and the new volume is 1L + 12 L = 13 L (V2), since the two containers are connected.
- Gases can be compressed into smaller volumes.
- Run the model, then change the volume of the containers and observe the change in pressure.
- What happens to the pressure when the volume changes?
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- As the pressure increases,
the volume of the container decreases.
- The
volume occupied by the gas particles is no longer negligible compared to the
volume of the container and the volume of the gas particles needs to be taken
into account.
- where P is the pressure, V is the volume, R is the universal gas constant, and T is the absolute temperature.
- Isotherm (plots of pressure versus volume at constant temperature) can be produced using the van der Waals model.
- The b term represents the excluded volume of the gas or the volume occupied by the gas particles.
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- Any amount of any substance will have a volume.
- If two water samples have different volumes, they still share a common measurement: the density.
- The density of a material is defined as its mass per unit volume.
- Density is calculated by the dividing the mass by the volume, so that density is measured as units of mass/volume, often g/mL.
- But how can he determine the volume of the crown?
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- At standard temperature and pressure, one mole of any gas will occupy a volume of 22.4 L.
- Stoichiometric calculations involving gases allow us to convert between mass, number of moles, and most importantly, volume of gases.
- 1 mole of any gas at standard temperature and pressure (273 K and 1 atm) occupies a volume of 22.4 L.
- Because we are told that the reaction takes place at STP, we can relate volume, 22.4 L, to 1 mol NO2.
- Calculate volumes of gases consumed/produced in a reaction using gas stoichiometry.
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- This is an important distinction; the volume in the definition of molarity refers to the volume of the solution, and not the volume of the solvent.
- Notice in the example above that volume must be converted to L from mL.
- Use molarity to convert between mass and volume in a solution.
- If you know the molarity, you can solve for either the number of moles or the volume of a solution.
- Translate between molarity, grams of solute in solution, and volume of solution.
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- Molarity is defined as the moles of a solute per volume of total solution.
- Then, we divide the number of moles by the total solution volume to get concentration.
- c1 and V1 are the concentration and the volume of the starting solution, which is the 5.0 M HCl. c2 and V2 are the concentration and the volume of the desired solution, or 150.0 mL of the 2.0 M HCl solution.
- The volume does not need to be converted to liters yet because both sides of the equation use mL.
- Notice that all of the units for volume have been converted to liters.