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
To solve this question, we can use Boyle's Law, which states that the pressure and volume of a gas are inversely proportional at constant temperature.
Boyle's Law can be expressed as: P₁V₁ = P₂V₂
We are given the initial pressure (P₁ = 200 kPa), the initial volume (V₁ = 15.0 L), and the final pressure (P₂ = 700 kPa). We need to find the final volume (V₂).
To find V₂, we can rearrange Boyle's Law equation: V₂ = (P₁V₁) / P₂
Substituting the given values:
V₂ = (200 kPa * 15.0 L) / 700 kPa
Calculating:
V₂ = 3000 / 700
V₂ ≈ 4.286 L
Rounded to two decimal places, 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 option c) 4.29 L.
To solve this problem, you can use Boyle's law, which states that the pressure and volume of a gas are inversely proportional when temperature and amount of gas are kept constant. The equation for Boyle's law is P₁V₁ = P₂V₂, where P₁ and V₁ are the initial pressure and volume, and P₂ and V₂ are the final pressure and volume.
Given:
Initial pressure (P₁) = 200 kPa
Initial volume (V₁) = 15.0 L
Final pressure (P₂) = 700 kPa (Note: there seems to be a typo in your question, stating "700 pka." I assume you meant "700 kPa.")
Final volume (V₂) = ?
Using Boyle's law, we can set up the equation as follows:
P₁V₁ = P₂V₂
Substituting the given values:
(200 kPa)(15.0 L) = (700 kPa)(V₂)
Solving for V₂:
V₂ = (200 kPa)(15.0 L) / (700 kPa)
V₂ = 3,000 kPa·L / 700 kPa
V₂ ≈ 4.29 L
Therefore, the volume occupied by the carbon monoxide when the pressure is increased to 700 kPa is approximately 4.29 L.
The correct answer is (c) 4.29 L.