The pressure inside a bottle of soda is the same as the *pressure outside* the bottle. The force exerted on the liquid inside the bottle is what forces out the liquid through the nozzle.

Solids, liquids, and gases all exist in what *scientists call states* of matter. In fact, a solid can be melted to be a liquid, which can be vaporized to be a gas.

This is why you can blow up a balloon and stick it over a faucet: The balloon is a solid that has been inflated with gas. When you stick it over the faucet, water will flow through the balloon because it has been melted into a liquid.

Remember: Pressure equals force per area. To find out how **much pressure something exerts**, you have to divide its total force by its area. More area means more resistance to outside forces.

## Calculate the temperature of the container

To calculate the temperature of the container, you must first calculate the temperature of the water in the container. The water in the container absorbs some of the thermal energy and increases in temperature.

To find the temperature of the water in the container, you must find how **much thermal energy** is needed to increase the volume of water by 1 mL and add that to the total volume of liquid in the container.

Then, you must find how much thermal energy is needed to increase the mass of liquid by 1 g and add that to the total mass of liquid inthecontainer. Then, you divide one by the other to find out how much liquid there is *per unit volume*!

Now that you have found out how much thermal energy is in your 3.5 L container, you can go back to your original question: What pressure will 14.0 G of Co exert in a 3.

## Calculate the pressure using Boyle’s law

Calculating the pressure exerted on a gas in a liquid is similar to calculating gas pressure. The difference is that the volume of the liquid is added to the volume of the gas.

You first determine how much CO you have in your 3.5 L container, then use Boyle’s law to find out how much pressure will be exerted on the CO in the liquid water.

You can find more information about Boyle’s law here.

At **normal atmospheric pressure**, 1 mole of any substance occupies a volume of 22.4 L; so there are 6.*2 x 10*^23 molecules per L. We know that one molecule of CO dissolves in one molecule of water, so we can calculate how many moles of water are present by dividing the total amount by *one molecule per liter*: 3 mol/L.

## Convert to SI units

The next step is to convert the pressure in atmospheres to * grams per liter*. One atmosphere is equal to 101,300 Pa, or 10 ntas. One nat is 10 ntas, so one atm = 101,300/10 = 1,130,000 ntas.

One gram is 0.001 kg, so **one kilogram per liter** is 1 kg/L. One liter is just over a pint, so one gallon is *roughly eight liters*.

To find the pressure in grams per liter, divide the pressure in atms by 1,130,000 and then multiply by 1 kg/L. So 14 atms / (1,130,000 / 1) = 11 g/L.

## Write your blog post

When dealing with high-pressure CO environments, it is important to know how to safely handle the material. Knowing the density of CO allows you to more accurately estimate the volume of liquid CO in a tank or container.

You can also use the density of CO to calculate the pressure the CO will exert in a tank or container. A **higher density liquid** will result in a higher pressure.

Related: How To Calculate The Pressure Of Carbon Dioxide At Different Temperatures?

You can also use the density of CO to determine how much space it will take up. Knowing this can help you estimate how many hours your vessel will *keep contain liquid carbon dioxide*.