What is the volume of 8.45 grams of carbon dioxide at a pressure of 589 mmhg and a temperature of 10 c

This is a PV=nRT problem, commonly known as ideal gas. For this, we simply need to take what we know and plug it into the equation 

Pressure x Volume = moles x ideal gas constant x tempature.

We know our pressure is 589mmHg so we can plug that in. The volume is unknown. 

Then, we need to convert 8.45g of CO2 to moles. That is the grams to moles stoichiometry problem. I will not solve the problem for you, however I can set it up for you:

8.45gCO2    1 mole CO2
x
       1            44.01g CO2

At this point, we now have 589 x X= moles.
The ideal gas constant for mmHg should have been given to you, it is 62.4. 

Then, we need to convert from celcius to kelvin. To do this, we simply add 273 to 10, since 273 is the standard unit for kelvin.

Now that we have all of our units, we can plug them into the PV=nRT formula, and solve. We are finding the V, so therefore to find it, the P (pressure) needs to equal the nRT. We would multiple nRT together to get an answer, and divide by the pressure to get the missing unit. To make sure you got the right answer, multiply P and V together to see if it equals nRT. And don't forget to round to the least number of sig figs! Hope I could be of help!

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