Question

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.)

Answer 1

The pressure inside the syringe will become approximately 2 atmospheres

Step-by-step 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.