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A sample of a gas has a volume of 1.5 L at 150 K. If the gas is heated to 235 K at constant pressure, what will its final volume be?

Initial conditions: V₁ = 1.5 L, T₁ = 150 K
Final conditions: V₂ = ? L, T₂ = 235 K

For a fixed amount of gas at constant pressure: V₁/T₁ = V₂/T₂
Then, V₂ = V₁ × (T₂/T₁)

Final volume, V₂ = (1.5 L) × (235/150) = 2.35 L


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A 3.0 L container holds a sample of oxygen gas at 1.5 atm pressure. If the pressure increases to 2.0 atm and the temperature remains constant, what is the new volume of the container?

Initial conditions: P₁= 1.5 atm, V₁ = 3.0 L
New conditions: P₂ = 2.0 atm. V₂ = ? L

For a fixed amount of gas at constant temperature: P₁V₁ = P₂V₂
Then, V₂ = V₁ × (P₁/P₂)

New volume, V₂ = (3.0 L) × (1.5/2.0) = 2.25 L

A sample of a gas has a volume of 1.5L at 150K. If the gas is heated to 235K at constant pressure, what will its final volume be?
use formula ... V1 T1 = V2 T2 <<< charles law ... 1s and 2s are subscripts ... just labels meaning 1st and 2nd
(1.5)(150) = V2 (235) <<< solve for V2
V2 = (1.5)(150)/(235) <<< use a calculator

A 3.0 L container holds a sample of oxygen gas at 1.5 atm pressure. If the pressure increases to 2.0 atm and the temperature remains constant, what is the new volume of the container?
Use Boyle's Law ... P1 V1 = P2 V2
(1.5)(3.0) = (2.0) V2 <<< solve for V2
V2 = (1.5)(3.0)/(2.0) <<< use a calculator