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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 was 760 torr, if the amount of gas does not change?

User Cshotton
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1 Answer

5 votes

Answer:

The amount of final volume when mass of the system is constant =

0.526 L

Step-by-step explanation:

Given data


V_(1) = 500 mL = 0.5 L


P_(1) = 740 torr


T_(1) = 25 ° c = 298 K


T_(2) = 50 ° c = 323 K


P_(2) = 760 torr

From ideal gas equation we get


P_(1) (V_(1) )/(T_(1) ) = P_(2) (V_(2) )/(T_(2) )


740 ((0.5)/(298) )= 760 ((V_(2) )/(323) )


V_(2) = 0.526 L = 526 ml

This is the amount of final volume when mass of the system is constant.

User DEBENDRA DHINDA
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