Question

Temperature in Kelvin does 60.5 liters of sulfur dioxide occupy if there are 2.5 mil at 0.75 atm

Answer 1

221.2 K.

Step-by-step explanation:

We would firstly need to identify sulfur dioxide as a gas. At low pressures and high temperatures, we may use the ideal gas law which states that:

`pV = nRT`

That is, the product between the pressure and the volume is equal to the product of moles, the ideal gas law constant and the absolute temperature.

Let's rearrange the equation for the absolute temperature dividing both sides of the equation by nR:

`(pV)/(nR)=T`

Substitute the variables. Given:

`V = 60.5 L, n = 2.5 mol, p = 0.75 atm, R = 0.08206 (L atm)/(mol K)`

We obtain:

`T=(0.75 atm\cdot60.5 L)/(0.08206(L atm)/(mol K)\cdot2.5 mol)=221.2 K`

In case the answer is preferred in Celsius, we may simply use the following conversion:

`T^(o)C=T(K)-273.15=221.2 K - 273.15 K=-52.0^(o)C`