A sample of gas has an initial volume of 2.4 L at a pressure of 855 mm Hg and a temperature of 298 K. If the gas is heated to a temperature of 387 K and expanded to a volume of 4.1 L, what is its final pressure in millimeters of mercury?

Question

Accepted Answer

GIVEN:

[latex]P_1[/latex] = 855 mm Hg

[latex]V_1[/latex] = 2.4 L

[latex]T_1[/latex] = 298 K

[latex]V_2[/latex] = 4.1 L

[latex]T_2[/latex] = 387 K

FIND: [latex] P_2[/latex]

RELATIONSHIPS USED

[latex] \frac{P_1V_1}{T_1}=\frac{P_2V_2}{T_2}[/latex] (Combined gas law, Section 11.6)

[latex] \frac{P_1V_1}{T_1}=\frac{P_2V_2}{T_2}\ P_2=\frac{P_1V_1T_2}{T_1V_2}\=\frac{855 mm Hg imes 2.4 \cancel{L} imes 387 \cancel{K}}{298 \cancel{K} imes 4.1 \cancel{L}} \ =6.5 imes 10^2 mm Hg[/latex]

The units, mm Hg, are correct. The value of the answer makes sense because the volume increase was proportionally more than the temperature decrease; therefore you would expect the pressure to decrease.

Question 11.15: A sample of gas has an initial volume of 2.4 L at a pressure......

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