A sample of gas in a balloon has a temperature of (+ 23.1oC), a current volume of 15.93 L and a pressure of 763 mmHg. If the balloon rises in the atmosphere and takes on a new volume of 45 .00 L at a pressure of 720 mmHg, what is the temperature at this altitude?

516°C is the temperature at this altitude.

Explanation:

The combined gas equation is,

where,

= initial pressure of gas in balloon = 763 mmHg

= final pressure of gas in balloon= 720 mmHg

= initial volume of gas in balloon= 15.93 L

= final volume of gas in balloon= 45.00L

= initial temperature of gas in balloon=

= final temperature of gas in balloon= ?

Now put all the given values in the above equation, we get:

516°C is the temperature at this altitude.

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: