# How many liters would 14.0 grams of chlorine gas occupy at 300.0 K and 1.51 atm?

##### 1 Answer

#### Explanation:

The first thing to do here is use the molar mass of chlorine gas to determine how many *moles* of chlorine gas you have in that sample.

#14.0color(red)(cancel(color(black)("g"))) * "1 mole Cl"_2/(70.906color(red)(cancel(color(black)("g")))) = "0.1974 moles Cl"_2#

Now that you know how many moles of gas you're dealing with, and the conditions for pressure andtemperature at which the gas is kept, you can use the ideal gas law equation to solve for the volume of the sample.

#color(blue)(PV = nRT)" "# , where

*universal gas constant*, usually given as

Rearrange this equation to solve for

#PV = nRT implies V = (nRT)/P#

#V = (0.1974color(red)(cancel(color(black)("moles"))) * 0.082(color(red)(cancel(color(black)("atm"))) * "L")/(color(red)(cancel(color(black)("mol"))) * color(red)(cancel(color(black)("K")))) * 300.0color(red)(cancel(color(black)("K"))))/(1.51color(red)(cancel(color(black)("atm")))) = "3.2159 L"#

Rounded to three sig figs, the answer will be

#V = color(green)("3.22 L")#