Open Question
Which assumptions of the kinetic–molecular theory explain the behavior of gases described by Boyle's law? Explain your answer.
11 Gases
Chemistry Gas Laws
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A 10.0 L cylinder with a movable piston exerts 3.00 atm of pressure. What will happen to the pressure if the volume of the container increases to 20.0 L?
a) It will double
b) It will decrease by half
c) It will increase slightly
d) No change
A
It will double
B
It will decrease by half
C
It will increase slightly
D
No change
Verified step by step guidance1
Identify the initial conditions: The initial volume (V1) is 10.0 L and the initial pressure (P1) is 3.00 atm.
Identify the final condition: The final volume (V2) is 20.0 L. We need to find the final pressure (P2).
Recall Boyle's Law, which states that for a given amount of gas at constant temperature, the pressure of a gas is inversely proportional to its volume. Mathematically, this is expressed as P1 * V1 = P2 * V2.
Substitute the known values into Boyle's Law equation: (3.00 atm) * (10.0 L) = P2 * (20.0 L).
Solve for P2 by dividing both sides of the equation by the final volume (20.0 L) to find the new pressure.
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