1- A sample of Ne(g) has a volume 250 mL at 752 mm Hg. What is the new volume if the temperature and amount of gas held constant, the
pressure is;
a) lowered to 385 mm Hg.
b) Increased to 3.68 atm

A. 488.31 mL.

B. 67.22 mL.

Explanation:

From the question given above, the following data were obtained:

Initial volume (V₁) = 250 mL

Initial pressure (P₁) = 752 mm Hg

A. Determination of the new volume when the pressure is lowered to 385 mmHg.

Initial volume (V₁) = 250 mL

Initial pressure (P₁) = 752 mm Hg

Final pressure (P₂) = 385 mmHg

Final volume (V₂) =?

P₁V₁ = P₂V₂

752 × 250 = 385 × V₂

188000 = 385 × V₂

Divide both side by 385

V₂ = 188000 / 385

V₂ = 488.31 mL

Thus, the new volume of the gas is 488.31 mL

B. Determination of the new volume of the gas when the pressure is increased to 3.68 atm.

Initial volume (V₁) = 250 mL

Initial pressure (P₁) = 752 mm Hg

Final pressure (P₂) = 3.68 atm.

Final volume (V₂) =?

Next, we shall convert 3.68 atm to mmHg. This can be obtained as follow:

1 atm = 760 mmHg

Therefore,

3.68 atm = 3.68 atm × 760 mmHg / 1 atm

3.68 atm = 2796.8 mmHg

Thus, 3.68 atm is equivalent to 2796.8 mmHg.

Finally, we shall determine the new volume of the gas as follow:

Initial volume (V₁) = 250 mL

Initial pressure (P₁) = 752 mm Hg

Final pressure (P₂) = 2796.8 mmHg.

Final volume (V₂) =?

P₁V₁ = P₂V₂

752 × 250 = 2796.8 × V₂

188000 = 2796.8 × V₂

Divide both side by 2796.8

V₂ = 188000 / 2796.8

V₂ = 67.22 mL

Thus, the new volume of the gas is 67.22 mL

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