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LuckyWell [14K]
3 years ago
15

Calculate the pressure, in atmospheres, required to compress a sample of helium gas from 27.3 L (at 1.00 atm) to 3.36 L at const

ant temperature. Enter your answer in the box provided. atm
Chemistry
1 answer:
inn [45]3 years ago
4 0

Answer:

8.125 atm

Explanation:

Hello,

Boyle's law states that at constant temperature:

P_1V_1=P_2V_2

In this case:

P_1=1 atm, V_1=27.3L, V_2=3.36L

Solving for P_2:

P_2=\frac{P_1V_1}{V_2}=\frac{1atm*27.3L}{3.36L}\\P_2=8.125atm

Best regards!

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Explanation:

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3 years ago
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Answer : The correct option is (A).

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