A sample of chlorine gas occupies a volume of 946 mL at a pressure of 726 mmHg. What is the pressure of the gas (in mmHg) if the volume is reduced at constant temperature to 154 mL?

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A sample of chlorine gas occupies a volume of 946 mL at a pressure of 726 mmHg. What is the pressure of the gas (in mmHg) if the volume is reduced at constant temperature to 154 mL?

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Answer 1 · 2016-12-12T17:49:33

$P_{2} ≅ 6 \cdot a t m .$ $P_2~=6*atm.$

Explanation:

$P_{1} V_{1} = P_{2} V_{2}$ $P_1V_1=P_2V_2$ at $constant temperature$ $"constant temperature"$ .

$P_2=(P_1V_1)/V_2=(946*cancel(mL)xx(726*cancel(mm*Hg))/(760*cancel(mm*Hg)*atm^-1))/(154*cancel(mL))=??atm$

Note that you do NOT measure a pressure that is over $1*atm$ in $mm*Hg$ . You do this and you will get mercury all over the laboratory. It's a big deal and a big, messy clean up job if you spill it.

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A sample of chlorine gas occupies a volume of 946 mL at a pressure of 726 mmHg. What is the pressure of the gas (in mmHg) if the volume is reduced at constant temperature to 154 mL?

1 Answer

Explanation:

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