A container of oxygen has a volume of 349 mL at a temperature of 22.0°C . What volume will the gas occupy at 50.0°C?

2 Answers
Nov 26, 2015

We assume a constant pressure. Thus Charles' Law applies.

Explanation:

Charles' Law states that at constant pressure, and constant amount of gas, volume is proportional to absolute temperature, i.e. #VpropT#.

So #V=kT#, where #V# = volume, #k# is some constant, and #T# is absolute temperature.

So, in each case, #V_1=kT_1, and V_2=kT_2#. If we solve for #k#, then #V_1/T_1 = V_2/T_2#.

Thus, #V_2=(V_1xxT_2)/T_1# #=# #(0.349*dm^3xx337cancelK)/(295cancelK)# #=# #??# #dm^3#

Note that #V_2# will be bigger (reasonably), because #T_2# has increased from #T_1#.

Nov 26, 2015

The final volume will be 382 mL.

Explanation:

Charles' law states that the volume of a given amount of a gas kept at constant pressure, is directly proportional to the temperature in Kelvins. http://chemistry.bd.psu.edu/jircitano/gases.html

The equation needed to solve this problem is #V_1/T_1=V_2/T_2#.

Given/Known
#V_1="349 mL"#
#T_1="22.0"^"o""C"+273.15="295.2 K"#
#T_2="50.0"^"o""C"+273.15="323.2 K"#

Unknown
#V_2#

Equation

#V_1/T_1=V_2/T_2#

Solution
Rearrange the equation to isolate #V_2# and solve.

#V_2=(V_1T_2)/T_1#

#V_2=(349"mL"xx323.2cancel"K")/(295.2cancel"K")="382 mL"#