Boyle's Law states that for a given amount of gas at a constant temperature, the volume of the gas is inversely proportional to the pressure exerted on it. This means that if the pressure increases, the volume decreases, and conversely, if the pressure decreases, the volume increases.
Here's how we arrive at the answer step by step:
1. Understanding Boyle's Law:
- Boyle's Law can be written as: [tex]\( P \times V = \text{constant} \)[/tex]
- Where [tex]\( P \)[/tex] is the pressure and [tex]\( V \)[/tex] is the volume.
- This implies [tex]\( V \propto \frac{1}{P} \)[/tex], meaning volume is inversely proportional to pressure.
2. Analyzing the Options:
- A) Kelvin temperature:
- Boyle’s Law does not mention temperature affecting the volume. It's only about pressure and volume at a constant temperature.
- B) Barometric pressure:
- Barometric pressure is the atmospheric pressure. According to Boyle's Law, as pressure increases, the volume of gas decreases when temperature is constant. Hence, the volume is inversely proportional to the pressure.
- C) Isoelectric mixture:
- An isoelectric mixture relates to chemistry and biochemistry topics, having no direct relation to the principles of Boyle's Law regarding the gas volume and pressure relationship.
- D) Vapor concentration:
- Vapor concentration generally pertains to the amount of vapor present in a mixture, which is not directly discussed in Boyle's Law regarding the inversely proportional relationship between volume and pressure.
3. Conclusion:
- The option which correctly fits Boyle’s Law, showcasing the inverse proportionality between pressure and volume, is Barometric Pressure.
Therefore, the correct answer is:
B) Barometric pressure
