1. To solve this problem, we can use the combined gas law equation, which states that P1V1/T1 = P2V2/T2, where P is pressure, V is volume, and T is temperature. Since the temperature remains constant, we can simplify the equation to P1V1 = P2V2. We know that the initial pressure is 0.95 atm and the initial volume is 1.5 L. To reduce the volume by 2, we need to end up with a volume of 1.5/2 = 0.75 L. Plugging in these values, we get:
[tex]0.95 \: atm \: x \: 1.5 L = P2 \: x \: 0.75 L[/tex]
Solving for P2, we get:
[tex]P2 = (0.95 \: atm \: x \: 1.5 L) / 0.75 L = 1.9 \: atm[/tex]
Therefore, the pressure needed to reduce the volume of oxygen gas by 2 is 1.9 atm.
2. To solve this problem, we can use the same combined gas law equation. We know that the initial volume is 6.00 L and the initial pressure is 1.01 atm. We want to compress this gas into a cylinder with a volume of 3.00 L. Plugging in these values, we get:
[tex]1.01 \: atm \: x \: 6.00 L = P2 \: x \: 3.00 L[/tex]
Solving for P2, we get:
[tex]P2 = (1.01 \: atm \: x \: 6.00 L) / 3.00 L = 2.02 \: atm[/tex]
Therefore, a pressure of 2.02 atm is needed to compress 6.00 liters of gas at 1.01 atmospheric pressure into a 3.00 liter cylinder.
Answers & Comments
HELLO FOLK
[tex]0.95 \: atm \: x \: 1.5 L = P2 \: x \: 0.75 L[/tex]
Solving for P2, we get:
[tex]P2 = (0.95 \: atm \: x \: 1.5 L) / 0.75 L = 1.9 \: atm[/tex]
Therefore, the pressure needed to reduce the volume of oxygen gas by 2 is 1.9 atm.
[tex]1.01 \: atm \: x \: 6.00 L = P2 \: x \: 3.00 L[/tex]
Solving for P2, we get:
[tex]P2 = (1.01 \: atm \: x \: 6.00 L) / 3.00 L = 2.02 \: atm[/tex]
Therefore, a pressure of 2.02 atm is needed to compress 6.00 liters of gas at 1.01 atmospheric pressure into a 3.00 liter cylinder.