At 82K, a gas has a volume of 4.60L. What would be the volume of the gas at 70K?

V₂ = 4.0L

Explanation:

Decreasing temperature => Decreasing Volume (Charles Law)

For a given volume, use a temperature ratio that will give a smaller volume.

Volume at lower temp = 4.6L(70K/82K) = 4.0L ... Using (82K/70K) would give a larger volume => contrary to temperature effects on gas volumes when pressure and mass are kept constant.

Pressure effects on Gas Volumes:

Note: The same idea is applied to pressure effects on gas volumes also except that changes in pressure affect gas volumes indirectly. That is, an increase in pressure => decrease in volume, or a decrease in pressure => increase in volume. Boyles Law => V ∝ 1/P.

Given a gas volume of 4.60L at 760mmHg, what is volume at 848mmHg?

Increasing pressure => Decreases Volume (Boyles Law)

For the given volume use a pressure ratio that will give a smaller volume.

Volume at higher pressure = 4.6L(760mm/848mm) =4.1L. Using (848mm/760mm) would give a larger volume => contrary to pressure effects on gas volume when temperature and mass of gas are kept constant.

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in 1783 cavendish was working with his hydrogen gas and found that when he burned it and condensed the vapor it was water. this was very significant since it disproved the greek theory of elements completely since water was not a simple substance but the product of two gases. it was lavoisier who hearing of the experiment gave cavendish's gas the name hydrogen ("water-producer") and added that hydrogen burned by combining with oxygen and that water was a hydrogen-oxygen combination.

explanation: