Suppose you have a syringe full of 30 ml 30 ml of normal air at atmospheric pressure. If you reduce the volume of the syringe to 19 ml 19 ml , what will the pressure inside the syringe become in atmospheres? (Do not include units in your answer. Round your answer to the nearest whole number.)

The pressure inside the syringe will become approximately 2 atmospheres

Explanation:

The question is about the relationship between pressure and volume, hence Boyle's law which states hat the volume of a given mass of gas is inversely proportional to its pressure, provided that the temperature remain constant.

That is P₁V₁ = P₂V₂

Where:

P₁ = Initial pressure = 1 atm

V₁ = Initial volume = 30 ml

P₂ = Final pressure  = Required

V₂ = Final volume = 19 ml

Plugging in the values, we have

1 atm × 30 ml= 19 ml ×P₂

∴ P₂ = 30 (atm·ml)/19 ml = 1.579 atm ≈2 atm rounded to the nearest whole number.