1. If 22.5 L of nitrogen at 748 mm Hg are compressed to 725 mm Hg at constant temperature. What is the new volume?
2. A gas with a volume of 4.0L at a pressure of 205kPa is allowed to expand to a volume of 12.0L. What is the pressure in the container if the temperature remains constant?
3. What pressure is required to compress 196.0 liters of air at 1.00 atmosphere into a cylinder whose volume is 26.0 liters?
23.2L
what is your question here? All of these can be solved with the combined gas law.
x=23.2 mm
x=23.2 mm
I'm sorry, but your statement "x=23.2 mm" is incomplete and lacks context. Please provide more information or a complete question so that I can assist you better.
To solve these questions, we can use Boyle's Law, which states that the pressure and volume of a gas are inversely proportional at constant temperature. Mathematically, this relationship can be represented 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.
Now let's solve each question step by step:
1. Question: If 22.5 L of nitrogen at 748 mm Hg are compressed to 725 mm Hg at constant temperature, what is the new volume?
To find the new volume, we can use Boyle's Law:
P1 * V1 = P2 * V2
Substituting the given values:
(748 mm Hg) * (22.5 L) = (725 mm Hg) * V2
We can rearrange the equation to solve for V2:
V2 = (P1 * V1) / P2
= (748 mm Hg * 22.5 L) / 725 mm Hg
= 23.207 L (rounded to three decimal places)
Therefore, the new volume is approximately 23.207 L.
2. Question: A gas with a volume of 4.0L at a pressure of 205kPa is allowed to expand to a volume of 12.0L. What is the pressure in the container if the temperature remains constant?
Using Boyle's Law:
P1 * V1 = P2 * V2
Substituting the given values:
(205 kPa) * (4.0 L) = P2 * (12.0 L)
Again, we rearrange the equation to solve for P2:
P2 = (P1 * V1) / V2
= (205 kPa * 4.0 L) / 12.0 L
= 68.333 kPa (rounded to three decimal places)
Therefore, the pressure in the container is approximately 68.333 kPa.
3. Question: What pressure is required to compress 196.0 liters of air at 1.00 atmosphere into a cylinder whose volume is 26.0 liters?
Using Boyle's Law:
P1 * V1 = P2 * V2
Substituting the given values:
(1.00 atm) * (196.0 L) = P2 * (26.0 L)
Rearranging the equation to solve for P2:
P2 = (P1 * V1) / V2
= (1.00 atm * 196.0 L) / 26.0 L
= 7.54 atm (rounded to two decimal places)
Therefore, the required pressure is approximately 7.54 atm.