A gas occupies #"67. cm"^3# at #9.38 × 10^4color(white)(l)"Pa"# and 22 °C. What is its volume at #10.6 × 10^5color(white)(l)"Pa"# and 29 °C?

So, it's always a good idea to start by making a note of what information is being provided by the problem.

In your case, you know that the initial sample of gas

• occupies a volume equal to #"67 cm"^3#
• has a temperature of #22^@"C"#
• has a pressure of #9.38 * 10^4"Pa"#

  You then go on to change the temperature to #29^@"C"# and the pressure to #10.6 * 10^5"Pa"#.

  Notice that no mention of number of moles was made. This means that you can assume it to be constant. So, if you start from the ideal gas law equation, you can say that

  #P_1 * V_1 = n * R * T_1 -># the initial state of the gas

  and

  #P_2 * V_2 = n * R * T_2 -># the final state of the gas

  Since #n# is constant, and #R# is the universal gas constant, you can rearrange these equations to isolate these two constant terms on one side

  #(P_1 * V_1)/T_1 = n * R" "# and #" "(P_2 * V_2)/T_2 = n * R#

  Notice that you have two expressions that are equal to the same value, #n * R#. This means that they are equal to each other as well.

  #(P_1 * V_1)/T_1 = (P_2 * V_2)/T_2 -># the combined gas law equation

  Now all you have to do is rearrange this to solve for #V_2#, the volume of the gas at the final state.

  Look what happens if you divide both sides of the equation by #P_2#

  #P_1/P_2 * V_1/T_1 = (color(red)(cancel(color(black)(P_2))) * V_2)/(T_2 * color(red)(cancel(color(black)(P_2))))#

  #P_1/P_2 * V_1/T_1 = V_2/T_2#

  Now multiply both sides by #T_2# to get #V_2# alone one one side of the equation

  #P_1/P_2 * T_2/T_1 * V_1 = V_2/color(red)(cancel(color(black)(T_2))) * color(red)(cancel(color(black)(T_2)))#

  Finally, you got

  #V_2 = P_1/P_2 * T_2/T_1 * V_1#

  Now plug in your values and solve for #V_2# - do not foget to convert the temperature from degrees Celsius to Kelvin!

  #V_2 = (9.38 * 10^4color(red)(cancel(color(black)("Pa"))))/(10.6 * 10^5color(red)(cancel(color(black)("Pa")))) * ((273.15 + 29)color(red)(cancel(color(black)("K"))))/((273.15 + 22)color(red)(cancel(color(black)("K")))) * "67 cm"^3#

  #V_2 = "6.0695 cm"^3#

  You need to round this off to two sig figs, the number of sig figs you have for the initial volume of the gas

  #V_2 = color(green)("6.1 cm"^3)#

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

#P_1 = 9.38 × 10^4 "Pa"#; #V_1 = "67. cm"^3#; #T_1 = "22 °C =(22 + 273.15) K = 295 K"# #P_2 = 10.6 × 10^5 "Pa"#; #V_2 = "?"#; #T_2 = "29 °C = (29 + 273.15) K = 302 K"#

Now we must rearrange the Combined Gas Law equation to get #V_2# by itself.

Step 1. Multiply both sides by #T_2#.

#(P_1V_1)/T_1 × T_2 = (P_2V_2)/(color(red)(cancel(color(black)(T_1)))) × color(red)(cancel(color(black)(T_2)#

#(P_1V_1T_2)/T_1 = P_2V_2#

Step 2. Divide both sides by #P_2#.

#(P_1V_1T_2)/(P_2T_1) = (color(red)(cancel(color(black)(P_2)))V_2)/color(red)(cancel(color(black)(P_2)#

#(P_1V_1T_2)/(P_2T_1) = V_2# or #V_2 = (P_1V_1T_2)/(P_2T_1)#

#V_2 = (P_1V_1T_2)/(P_2T_1) = (9.38 × 10^4 color(red)(cancel(color(black)("Pa"))) × "67. cm"^ 3 × 302 color(red)(cancel(color(black)("K"))))/( 10.6 × 10^5 color(red)(cancel(color(black)("Pa"))) × 295 color(red)(cancel(color(black)("K")))) = "6.1 cm"^3#

The new volume should be about one-tenth of the original volume, or about #"7 cm"^3#.