The thing to remember here is that every time the temperature of a gas and the number of moles of gas are kept constant, the pressure and the volume of the gas have an inverse relationship described by Boyle's Law.
#color(blue)(ul(color(black)(P_1V_1 = P_2V_2)))#
#P_1#and #V_1#represent the pressure and volume of the gas at an initial state
#P_2#and #V_2#represent the pressure and volume of the gas at a final state
In your case, the pressure of the gas is increasing
#"118 kPa " -> " 214 kPa"#
so you should expect the volume of the gas to decrease
#"4 L " > color(white)(.)V_2#
Rearrange the equation to solve for
#P_1V_1 = P_2V_2 implies V_2 = P_1/P_2 * V_1#
Plug in your values to find
#V_2 = (118 color(red)(cancel(color(black)("kPa"))))/(214color(red)(cancel(color(black)("kPa")))) * "4 L" = color(darkgreen)(ul(color(black)("2 L")))#
The answer must be rounded to one significant figure, the number of sig figs you have for the initial volume of the gas.