Question

At constant temperature, a sample of helium at 760. torr in a closed container was compressed 5) from 5.00 L to 3.00 L, with no change in amount of gas or temperature. What was the new pressure exerted by the helium on its container?

A) 3820 torr
B) 1270 torr
C) 800.torr
D)15.0 torr
E) 2280 torr

Answer 1

B) 1270 torr

Step-by-step explanation:

Given data

• Initial volume (V₁): 5.00 L

• Initial pressure (P₁): 760 torr

• Final volume (V₂): 3.00 L

• Final pressure (P₂): ?

We can find the final pressure using Boyle's law.

P₁ × V₁ = P₂ × V₂

P₂ = P₁ × V₁/V₂

P₂ = 760 torr × 5.00 L/3.00 L

P₂ = 1.27 × 10³ torr = 1270 torr

The final pressure is 1270 torr.