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According to Boyle's Law, which describes the relationship between the volume and pressure of a gas at constant temperature, if the volume of a gas is decreased while the pressure is held constant, the temperature of the gas will increase.
Mathematically, Boyle's Law can be expressed as:
\[ PV = \text{constant} \]
where \( P \) is the pressure, \( V \) is the volume, and the product \( PV \) remains constant as long as the temperature is constant.
If you decrease the volume (\( V \)), according to Boyle's Law, the pressure (\( P \)) will increase. As a result, since the temperature is held constant in this scenario, there is an inverse relationship between volume and pressure. If one increases, the other must decrease to keep the product \( PV \) constant.
It's important to note that Boyle's Law holds true for ideal gases under the specified conditions. In real-world situations, factors like the compressibility of the gas and deviations from ideal behavior might influence the results.
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