A 10.0 g sample of carbon monoxide, a poisonous gas produced by the incomplete combustion of hyrdocarbons, occupies 15.0 l at a pressure of 200 kpa. the volume occupied by the carbon monoxide when the pressure is increased is 700 pka is
a) 1.16 L
b)4.05 L
c)4.29 L
d)52.5 L
P1V1 = P2V2
Substitute
(15.0 * 200)/ (700)
= 4.29 L
P1V1 = P2V2
13.5
To solve this problem, you can use Boyle's Law, which states that the pressure and volume of a gas are inversely proportional at constant temperature. This can be expressed as:
P1 * V1 = P2 * V2
Where P1 and V1 are the initial pressure and volume, and P2 and V2 are the final pressure and volume.
In this case, you are given the initial pressure (P1 = 200 kPa), initial volume (V1 = 15.0 L), and final pressure (P2 = 700 kPa). You need to find the final volume (V2).
Rearranging the equation, we can solve for V2:
V2 = (P1 * V1) / P2
Substituting the given values:
V2 = (200 kPa * 15.0 L) / 700 kPa
V2 = 3,000 / 700
V2 ≈ 4.29 L
So, the volume occupied by the carbon monoxide when the pressure is increased to 700 kPa is approximately 4.29 L.
Therefore, the correct answer is c) 4.29 L.