What is the volume, in liters, occupied by 0.723 mol of a gas at 32.0°C if the pressure is 852 mm Hg?

1 Answer
Jun 10, 2016

Answer:

the volume will be #V = 16.2L#

Explanation:

To solve for the volume we can use the Ideal Gas Law equation

#PV=nRT#

#P=# Pressure in #atm#
#V=# Volume in #L#
#n=# moles
#R=# the Gas Law Constant #0.0821 (atm*L)/(mol*K)#
#T=# Temperature in #K#

When using the Ideal Gas Law Constant we must convert the Pressure to #atm#
#P=852mmHg*(1atm)/(760mmHg)= 1.12 atm#

#V=?#

#n=0.723mol#

#R=0.0821 (atm*L)/(mol*K)#

When using the Ideal Gas Law Constant we must convert the Temperature to #K#
#T=32.0^oC+273 = 305K#

#V=(nRT)/P#

#V=((0.723cancel(mol))(0.0821 (cancel(atm)*L)/(cancel(mol)*cancel(K)))(305cancelK))/(1.12cancel(atm))#

#V = 16.2L#