A sample of gas at 53.0 oC and 1.19 atm occupies a volume of 2.3 L. What volume would this gas occupy at 107 oC and 0.60 atm?

Explanation:

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In this case, according to the given pressure, temperature and volume, it is possible for us to calculate the final volume via the combined ideal gas law:

In such a way, we solve for the final volume, V2, to obtain:

Then, we plug in the given data to obtain:

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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: