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A ball with a volume of 1.0 L is filled with a gas at 5 atmospheres (atm). If the volume is reduced to 0.75 L without a change in temperature, what would be the pressure of the balloon? ​

Sagot :

Lanuel

Answer:

P2 = 6.67 atm

Explanation:

Given the following data;

Initial volume = 1 Liters

Initial pressure = 5 atm

Final volume = 0.75 Liters

To find the final pressure P2, we would use Boyles' law.

Boyles states that when the temperature of an ideal gas is kept constant, the pressure of the gas is inversely proportional to the volume occupied by the gas.

Mathematically, Boyles law is given by;

[tex] PV = K[/tex]

[tex] P_{1}V_{1} = P_{2}V_{2} [/tex]

Substituting into the equation, we have;

[tex] 5 * 1 = P_{2} * 0.75 [/tex]

[tex] 5 = 0.75_{2} [/tex]

[tex] P_{2} = \frac {5}{0.75}[/tex]

[tex] P_{2} = 6.67[/tex]

P2 = 6.67 atm

Therefore, the new pressure is 6.67 atm.

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