Imagine that you have an ideal gas in a 6.70 L container, and that 1450 molecules of this gas collide with a square-inch area of the container at any given instant. If the volume is increased to 40.2 L at constant temperature, how many collisions will occur per square inch of this larger container? Enter the number of collisions per square inch

Question

Camron Bond

Chemistry

6 August, 13:58

Imagine that you have an ideal gas in a 6.70 L container, and that 1450 molecules of this gas collide with a square-inch area of the container at any given instant. If the volume is increased to 40.2 L at constant temperature, how many collisions will occur per square inch of this larger container? Enter the number of collisions per square inch

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Answers (1)

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Emmett Webster · Answer 1

they could collide 241.66 molec / in² by increasing the volume to 40.2L

Explanation:

ideal gas:

Boyle Law: at constant temperature the pressure of a gas varies inversely with the volume

V1 * P1 = V2 * P2 P = F / A

∴ V1 = 6.70 L;

∴ P1 = 1450 molec / in²

∴ V2 = 40.2 L

⇒ P2 = ((6.70 L) * (1450 molec/in²)) / 40.2 L

⇒ P2 = 241.66 molec/in²