Question

A CERTAIN MASS OF CHLORINE GAS OCCUPIES 750CM3 AT CERTAIN PRESSURE , WHEN THE PRESSURE WAS CHANGEFD TO 2.5 ATMOSPHERE , IT OCCUPIED 1500CM3, WHAT WAS THE INITIAL PRESURE IF THE TEMPERATURE WAS KEPT CONSTANT DURING COMPLETE OPERATION?

Answer 1

Given

• Initial volume of the gas (V₁) = 750 cm³
• Final volume of the gas (V₂) = 1500 cm³
• Final pressure of the gas (P₂) = 2.5 atm

To find

• Initial pressure of the gas (P₁)

Solution

☯ According to Boyles Law

• P₁ V₁ = P₂ V₂

• Let P₁ be x

☯ According to the question

• x × 750 = 2.5 × 1500

• x = 2.5 × ¹⁵⁰⁰⁄₇₅₀

• x = 2.5 × ²⁄₁

• x = 5

☯ The initial pressure of the gas is 5 atm

Answer 2

Explanation:

A CERTAIN MASS OF CHLORINE GAS OCCUPIES 750CM3 AT CERTAIN PRESSURE , WHEN THE PRESSURE WAS CHANGEFD TO 2.5 ATMOSPHERE , IT OCCUPIED 1500CM3, WHAT WAS THE INITIAL PRESURE IF THE TEMPERATURE WAS KEPT CONSTANT DURING COMPLETE OPERATION?