Question

A person has a 1.43mol sample of carbon dioxide. If the pressure if the sample is 34.56kpa, and the volume is 440.99mL, what will the temperature of the sample be in Kelvin?

Answer 1

`1.28K\text{ }`

Step-by-step explanation:

Here, we want to get the temperature of the gas

We can use the ideal gas equation here

Mathematically, we have this as:

`PV\text{ = nRT}`

P is the pressure which is given as 34.56 kPa

V is the volume which is given as 440.99 mL

R is the molar gas constant which is 0.08205 L atm/mol k

n is the number of moles which is given as 1.43 mol

We need to convert the pressure to the correct unit (considering the molar gas consnat value in atm)

1 kPa = 0.00986923 atm

34.56 kPa will be = 34.56 * 0.00986923 = 0.341 atm

We need to convert the volume to Liters by dividing by 1000

We have that as 440.99/1000 = 0.44099 L

Finally,we rewrite the equation in terms of temperature and substitute the values as follows:

`\begin{gathered} T\text{ = }(PV)/(nR) \\ \\ T\text{ = }(0.341*0.44099)/(1.43*0.08205)\text{ =1.28 K } \end{gathered}`