Question

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?

Answer 1

Answer:

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

0.526 L

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

$P_{1} \frac{V_{1} }{T_{1} } = P_{2} \frac{V_{2} }{T_{2} }$

$740 (\frac{0.5}{298} )= 760 (\frac{V_{2} }{323} )$

$V_{2} =$ 0.526 L =  526 ml

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