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

Explanation:

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

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

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

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

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