Assume that you have a cylinder with a movable piston. what would happen to the gas pressure inside the cylinder if you do the following? part a: decrease the volume to one-fourth the original volume while holding the temperature constant. express your answer in terms of the variable p initial. part b: reduce the kelvin temperature to half its original value while holding the volume constant. express your answer in terms of the variable p initial .part c: reduce the amount of gas to half while keeping the volume and temperature constant. express your answer in terms of the variable p initial .

A. The pressure will increase 4 times. P₂ = 4 P₁

B. The pressure will decrease to half its value. P₂ = 0.5 P₁

C. The pressure will decrease to half its value. P₂ = 0.5 P₁

Explanation:

Initially, we have n₁ moles of a gas that occupy a volume V₁ at temperature T₁ and pressure P₁.

What would happen to the gas pressure inside the cylinder if you do the following?

Part A: Decrease the volume to one-fourth the original volume while holding the temperature constant. Express your answer in terms of the variable P initial.

V₂ = 0.25 V₁. According to Boyle's law,

P₁ . V₁ = P₂ . V₂

P₁ . V₁ = P₂ . 0.25 V₁

P₁ = P₂ . 0.25

P₂ = 4 P₁

Part B: Reduce the Kelvin temperature to half its original value while holding the volume constant. Express your answer in terms of the variable P initial.

T₂ = 0.5 T₁. According to Gay-Lussac's law,

Part C: Reduce the amount of gas to half while keeping the volume and temperature constant. Express your answer in terms of the variable P initial.

n₂ = 0.5 n₁.

P₁ in terms of the ideal gas equation is:

P₂ in terms of the ideal gas equation is:

it’s previous models   because when i picked that son of a gun’s answer it was wrong look for previous models because they might make it a different letter