Would you expect the pressure of a 12.5 mL syringe of natural gas to be the same as the pressure of 12.5 mL of air? In other words, is Boyle's Law dependent on the type of gas that is being measured?
For an ideal gas Boyle's Law is independent of the kind of gas.
Yes
To determine whether the pressure of a 12.5 mL syringe of natural gas would be the same as the pressure of 12.5 mL of air, we need to consider Boyle's Law. Boyle's Law states that at a constant temperature, the pressure and volume of a gas are inversely proportional. In other words, as the volume decreases, the pressure will increase, and vice versa.
Boyle's Law is not dependent on the type of gas being measured; it applies to all gases as long as the temperature remains constant. Therefore, we can expect the pressure of a 12.5 mL syringe of natural gas to follow the same relationship as a 12.5 mL syringe of air.
If we want to calculate the pressure of the syringes, we need more information such as the initial volume and pressure of the gas, as well as the temperature. Once we have that information, we can use the formula of Boyle's Law:
P₁V₁ = P₂V₂
Where P₁ and V₁ are the initial pressure and volume, and P₂ and V₂ are the final pressure and volume. Given the volume of 12.5 mL for both syringes, we can compare the pressures by plugging the values into the equation and solving for the pressures.
In summary, based on Boyle's Law, the pressure of a 12.5 mL syringe of natural gas and a 12.5 mL syringe of air would follow the same relationship, and Boyle's Law is independent of the type of gas being measured. To calculate the pressure, more specific information about each gas and the conditions is necessary.