A student collects #450# #mL# of #HCl (g)# at a pressure of #100# #kPa# and a temperature of #17°C#. What is the new volume of the #HCl# at standard temperature and pressure?

1 Answer
David G.
Mar 28, 2016

Take #V_1/T_1=V_2/T_2# and rearrange to:

#V_2=(V_1T_2)/T_1=(0.450xx273)/290=0.424# #L# = #424# #mL#.

Explanation:

First convert the temperature to kelvin: #17+273=290# #K#. Standard temperature is #273# #K#.

Now #100# #kPa# is already standard pressure, so the pressure is constant.

We should work in SI units, so #450# #mL# = #0.450# #L#.

From the Combined Gas Law, but with pressure omitted because it is constant, take #V_1/T_1=V_2/T_2# and rearrange to #V_2=(V_1T_2)/T_1=(0.450xx273)/290=0.424# #L# = #424# #mL#.

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