The question is missing information. Here is the complete question.
A gas at a pressure of 2.0 atm is in a closed container. Indicate the changes (if any) in its volume when the pressure undergoes the following changes at constant temperature and constant amount of gas. Match the words in the left with the column to the appropriate blanks in the sentences on the right. Make certain each sentence is complete before submitting your answer.
1. The pressure increases to 6.0 atm. The volume ________
2. The pressure drops to 0.40 atm. The volume _________
3. The pressure remains at 2.0 atm. The volume _________
Answer: 1. Decreases
2. Increases
3. Does not change
Explanation: According to the Ideal Gas Law, <u>Pressure</u>, <u>Volume</u> and <u>Temperature</u> of an ideal gas is related, as the following: PV = nRT.
In this case, since temperature (T) and amount of gas (n) are constant, the <em><u>Boyle's</u></em> <em><u>Law</u></em> can be used.
The law states that the volume of a given gas, under the conditios of temperature and amount of it are constant, is inversely proportional to the applied pressure: P₁.V₁ = P₂.V₂
Initial P (P₁) = 2
Initial V (V₁) = V
Final P (P₂) = 6
P₁.V₁ = P₂.V₂
2.V = 6.V₂
V₂ = 1/3V
When the pressure increases to 6 atm, volume <em><u>decreases</u></em> by 1/3.
P₁ = 2
V₁ = V
P₂ = 0.4
2.V = 0.4V₂
V₂ = 5V
When pressure drops to 0.4 atm, volume <em><u>increases</u></em> by 5.
Since there are no change in the pressure, the volume is the same from the beginning, so <em><u>does not change</u></em>.
