We have to calculate the total pressure in the container when 5.60 g of solid CO_{2} evaporates into it.

The **pressure** of a particular mass of a gas can be calculated by the **ideal gas equation**:

$\overline{){\mathbf{PV}}{\mathbf{}}{\mathbf{=}}{\mathbf{}}{\mathbf{nRT}}}$

**Where,**

P = pressure

V = volume

n = number of moles

R = gas constant = 0.08206 L•atm/mol•K

T = temperature in Kelvin units

**We can ****rearrange this formula for pressure.**

$\overline{){\mathbf{P}}{\mathbf{}}{\mathbf{=}}{\mathbf{}}\frac{\mathbf{nRT}}{\mathbf{V}}}$

A piece of solid carbon dioxide with a mass of 5.60 g is placed in a 10.0-L vessel that already contains air at 710 torr and 24 °C.

After the carbon dioxide has totally vaporized, what is the total pressure in the container at 24 ^{o}C?

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