A sample of nitrogen occupies 11.2 liters under a pressure of 580 torr at 32◦C. What volume would it occupy at 32◦C if the pressure were increased to 700 torr?
To solve this problem, we can use Boyle's Law, which states that the volume of a gas is inversely proportional to its pressure, assuming temperature remains constant.
Boyle's Law can be written as:
P₁V₁ = P₂V₂
Where:
P₁ = initial pressure
V₁ = initial volume
P₂ = final pressure (given)
V₂ = final volume (unknown)
In this case, we are given:
P₁ = 580 torr
V₁ = 11.2 liters
P₂ = 700 torr
V₂ = ?
We can plug in the known values and solve for V₂:
P₁V₁ = P₂V₂
580 torr * 11.2 L = 700 torr * V₂
To isolate V₂, we can divide both sides of the equation by 700 torr:
(580 torr * 11.2 L) / 700 torr = V₂
Calculating this expression will give us the volume V₂ in liters.