Question

The pressure of a certain amount of gas in a 1.25 L balloon is 760 torr. What would the pressure of that balloon be if it's volume was increased to 2.15 L?

Answer 1

440 torr

General Formulas and Concepts:

Chemistry

Ideal Gas Law

Boyle's Law: P₁V₁ = P₂V₂

• P₁ is pressure
• V₁ is volume
• P₂ is new pressure
• V₂ is new volume

Math

Pre-Algebra

Order of Operations: BPEMDAS

1. Brackets
2. Parenthesis
3. Exponents
4. Multiplication
5. Division
6. Addition
7. Subtraction

• Left to Right

Equality Properties

• Multiplication Property of Equality
• Division Property of Equality
• Addition Property of Equality
• Subtraction Property of Equality

Step-by-step explanation:

Step 1: Define

Identify

[Given] V₁ = 1.25 L

[Given] P₁ = 760 torr

[Given] V₂ = 2.15 L

[Solve] P₂

Step 2: Solve for P₂

1. Substitute in variables [Boyle's Law]: (760 torr)(1.25 L) = P₂(2.15 L)
2. Multiply: 950 torr · L = P₂(2.15 L)
3. [Division Property of Equality] Divide 2.15 L on both sides: 441.86 torr = P₂
4. Rewrite: P₂ = 441.86 torr

Step 3: Check

Follow sig fig rules and round. We are given 2 sig figs as our lowest.

441.86 torr ≈ 440 torr