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?
Answers
Answered by
50
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
Answered by
11
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?
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