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At constant temperature, a sample of helium at 760. torr in a closed container was compressed from 5.00 l to 3.00 l. What was the new pressure exerted by the helium on its container?
Accepted Answer
This is a classic example of Boyle's Law, which states that the pressure and volume of a gas are inversely proportional at constant temperature. We can use the formula P₁V₁ = P₂V₂ to solve for the new pressure (P₂).
Here's how it works:
P₁ = 760 torr (initial pressure)
V₁ = 5.00 L (initial volume)
V₂ = 3.00 L (final volume)
Plugging these values into the equation:
760 torr
5.00 L = P₂
3.00 L
Solving for P₂:
P₂ = (760 torr
5.00 L) / 3.00 L = 1266.67 torr
Therefore, the new pressure exerted by the helium is approximately 1267 torr.
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