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?
A) 530 mL
B) 450 ml
C) 970 mL
D) 240 ml
E) 400 mL

Answer 1

Answer:  Thus the new volume of the gas is 530  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,

$\frac{P_1V_1}{T_1}=\frac{P_2V_2}{T_2}$

where,

$P_1$ = initial pressure of gas =  740 torr

$P_2$ = final pressure of gas = 760 torr

$V_1$ = initial volume of gas = 500 ml

$V_2$ = final volume of gas = ?

$T_1$ = initial temperature of gas = $25^oC=273+25=298K$

$T_2$ = final temperature of gas = $50^oC=273+50=323K$

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

$\frac{740\times 500}{298}=\frac{760\times V_2}{323}$

$V_2=530ml$

Thus the new volume of the gas is 530 ml