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A sample of nitrogen gas had a volume of 500. mL, a pressure in its closed container of 740 torr, and a temperature of 25 °C. What was the new volume of the gas when the temperature was changed to 50 °C and the new pressure is 760 torr

Respuesta :

Answer : The new volume of gas was, 523 mL

Explanation :

Combined gas law is the combination of Boyle's law, Charles's law and Gay-Lussac's law.

The combined gas equation is,

[tex]\frac{P_1V_1}{T_1}=\frac{P_2V_2}{T_2}[/tex]

where,

[tex]P_1[/tex] = initial pressure of gas = 740 torr

[tex]P_2[/tex] = final pressure of gas = 760 torr

[tex]V_1[/tex] = initial volume of gas = 500 mL

[tex]V_2[/tex] = final volume of gas = ?

[tex]T_1[/tex] = initial temperature of gas = [tex]25^oC=273+25=298K[/tex]

[tex]T_2[/tex] = final temperature of gas = [tex]50^oC=273+50=320K[/tex]

Now put all the given values in the above equation, we get:

[tex]\frac{740torr\times 500mL}{298K}=\frac{760torr\times V_2}{320K}[/tex]

[tex]V_2=522.78torr\approx 523mL[/tex]

Thus, the new volume of gas was, 523 mL

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