Question

An ideal gas originally at 0.85 atm and 66°C was allowed to expand until its final volume, pressure and temperature were 94.0mL, 456 mmHg and 113°F. What was the original volume in liters?

Answer 1

Answer: The original volume in liters was 0.0707L

Step-by-step explanation:

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

The combined gas equation is,

`(P_1V_1)/(T_1)=(P_2V_2)/(T_2)`

where,

`P_1` = initial pressure of gas = 0.85 atm

`P_2` = final pressure of gas = 456 mm Hg = 0.60 atm (760mmHg=1atm)

`V_1` = initial volume of gas = ?

`V_2` = final volume of gas = 94.0 ml

`T_1` = initial temperature of gas =
`66^oC=273+66=339K`

`T_2` = final temperature of gas =
`113^oF=318K`
`(32^0F=273K)`

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

`(0.85* V_1)/(339)=(0.60* 94.0)/(318)`

`V_1=70.7ml=0.0707L` (1L=1000ml)

Thus the original volume in liters was 0.0707L