The statement which represents Boyle's Law for a constant temperature is: A) decreasing volume of gas increases pressure exerted by the gas
Robert Boyle was an Irish chemist and is famously referred to as the first modern chemist. He was born on the 25th of January, 1627 in Lismore, Ireland and died on the 31st, December 1691, London, United Kingdom.
Boyle's states that when the temperature of an ideal gas is kept constant, the pressure of the gas is inversely proportional to the volume occupied by the gas.
Mathematically, Boyle's law is given by the formula;
[tex]PV = k\\\\P_{1}V_{1} = P_{2}V_{2}[/tex]
Where;
- [tex]P_{1}[/tex] is the original (initial) pressure.
- [tex]P_{2}[/tex] is the final pressure.
- [tex]V_{1}[/tex] is the original (initial) volume.
- [tex]V_{2}[/tex] is the final volume.
According to Boyle's law, when the volume of a gas is decreased at a constant temperature, the pressure exerted by the gas is increased and when the volume of a gas is increased at a constant temperature, the pressure exerted by the gas is decreased because of the inverse relationship between them.
In conclusion, decreasing volume of gas increases pressure exerted by the gas provided temperature of the gas is kept constant in accordance with Boyle's law.
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