Recall the **ideal gas law equation**

*Where:*

P , pressure = **895 torr**

n , number of moles, unknown

V , volume =** 8.7 L**

**R, gas constant =**

*** Values for the gas constant can be found online or in textbooks** *

T, temperature in K, but given: *T = 24**°C*

__To solve for grams of Cl_{2}, we need to do these steps:__

- Convert:
- Temperature from
*°C to K* - Pressure from torr to atm

- Temperature from
- Solve for the
**molar mass of Cl**_{2} - Solve for
**n, moles of Cl**_{2 }*using Ideal Gas Law* - Do a
**mole to mass**calculation

Chlorine is widely used to purify municipal water supplies and to treat swimming pool water. Suppose that the volume of a particular sample of Cl_{2} gas is 8.70 L at 895 torr and 24 ^{o}C.

How many grams of Cl_{2} are in the sample?