S1 .4 - Quantitative chemistry

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8 Terms

1
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Avogadro constant

number of 12 C atoms in exactly 12.00g of 12C, = 6.02 x 1023

2
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ideal gas

All collisions between particles (in constant, random motion) are perfectly elastic

no intermolecular forces between the particles

particles have negligible volume

The temperature of the gas is proportional to the average kinetic energy of its particles, and the pressure is due to collisions of the particles with the vessel walls.

3
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real gas

Some attractive forces between the particles and the particles themselves do occupy some space
can condense into liquid
will behave ideally in high temperatures and low pressures

4
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Boyle's Law

P∝1/V , At constant temperature: as the volume decreases the concentration of the particles increases, resulting in more collisions with the container walls. The increase in pressure is inversely proportional to the decrease in volume, i.e. doubling the pressure halves the volume

<p><span>P∝</span>1/<span>V</span> , At constant temperature: as the volume decreases the concentration of the particles increases, resulting in more collisions with the container walls. The increase in pressure is inversely proportional to the decrease in volume, i.e. doubling the pressure halves the volume</p>
5
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Charles's Law

V∝T, At constant pressure: at higher temperatures, the particles have a greater average velocity so individual particles collide with the container walls with greater force. To keep the pressure constant there must be fewer collisions per unit area so the volume of the gas must increase. The increase in volume is directly proportional to the absolute temperature, i.e. doubling the absolute temperature doubles the volume.

<p>V∝T, At constant pressure: at higher temperatures, the particles have a greater average velocity so individual particles collide with the container walls with greater force. To keep the pressure constant there must be fewer collisions per unit area so the volume of the gas must increase. The increase in volume is directly proportional to the absolute temperature, i.e. doubling the absolute temperature doubles the volume.</p>
6
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Gay-Lussac's Law

P∝T, At constant volume: increasing the temperature increases the average kinetic energy, so the force with which the particles collide with the container walls increases. Hence pressure increases and is directly proportional to the absolute temperature, i.e. doubling the absolute temperature doubles the pressure.

7
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Avogadro's law (molar volume of gases)

Avogadro's law states that equal volumes of different gases at the same temperature and pressure contain the same number of moles.

One mole of any gas will occupy the same volume at the same temperature and pressure. at STP: 22.7 × 10-2m3

8
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atom economy

a measure of the amount of starting materials that become useful products

<p>a measure of the amount of starting materials that become useful products</p>