Question

How many grams of chlorine would exert a pressure of 610 torr in a 3.26-liter container at standard temperature? 4.25gCL

Answer 1

`m=8.28gCl_2`

Step-by-step explanation:

Hello there!

In this case, according to the given information, it possible for us to realize that this problem is solved via the ideal gas equation:

`PV=nRT`

By which we solve for the moles of chlorine gas as shown below:

`n=(PV)/(RT)`

Next, we plug in the given pressure (in atm), the volume and standard pressure (273.15K) to obtain:

`n=(610/760atm*3.26L)/(0.08206(atm*L)/(mol*K)*273.15K)\\\\n=0.117molCl_2`

Then, since the molar mass of chlorine gas (Cl2) is 70.9 g/mol, the mass of this gas turns out to be:

`m=0.117molCl_2*(70.9gCl_2)/(1molCl_2) \\\\m=8.28gCl_2`

Regards!