Question

A large balloon is initially filled to a volume of 11.2 L at 325 K and a pressure of 3450 mm Hg. What volume of gas will the balloon contain at 1.4 atm and 325 K?

Answer 1

36 L

Step-by-step explanation:

Since the temperature remains constant, you can use Boyle's Law to find the final volume:

P₁V₁ = P₂V₂

In this formula, "P₁" and "V₁" represent the initial pressure and volume. "P₂" and "V₂" represent the final pressure and volume. Before, you can plug the given values into the equation and solve for "V₂", you need to convert mmHg to atm to maintain consistent units.

760 mmHg = 1 atm

P₁ = 3,450 mmHg / 760 mmHg = 4.54 atm P₂ = 1.4 atm

V₁ = 11.2 L V₂ = ? L

P₁V₁ = P₂V₂ <----- Boyle's Law

(4.54 atm)(11.2 L) = (1.4 atm)V₂ <----- Insert values

50.848 = (1.4 atm)V₂ <----- Multiply 4.54 and 11.2

36 = V₂ <----- Divide both sides by 1.4