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?

440 torr

General Formulas and Concepts:

Chemistry

Ideal Gas Law

Boyle's Law: P₁V₁ = P₂V₂

P₁ is pressureV₁ is volumeP₂ is new pressureV₂ is new volume

Math

Pre-Algebra

Order of Operations: BPEMDAS

Brackets Parenthesis Exponents Multiplication Division Addition Subtraction Left to Right  

Equality Properties

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

Substitute in variables [Boyle's Law]:                                                              (760 torr)(1.25 L) = P₂(2.15 L)Multiply:                                                                                                             950 torr · L = P₂(2.15 L)[Division Property of Equality] Divide 2.15 L on both sides:                          441.86 torr = P₂Rewrite:                                                                                                             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

No is the answer to the question