Question

• If I have 5.4 moles of a gas at a pressure of 2.3 atm and a volume of 14 liters, what is thetemperature in Kelvin?

Answer 1

For this exercise we assume ideal gas to use the ideal gas law:

p x V = n x R x T (1)

From this equation, we clear T, where:

p = pressure in atm

V = volume in L

n = moles

T = temperature in K

R = gas constant (we can find this on books, the Internet, and even students can ask the teacher about its value)

R in this case and because of units is equal to 0.082 atm x L / mol x K

Procedure:

`\begin{gathered} p\text{ x V = n x R x T } \\ \frac{p\text{ x V}}{n\text{ x R}}=\text{ T} \\ \frac{2.3\text{ atm x 14 L}}{5.4\text{ moles x 0.082 }\frac{atm\text{ L}}{\text{mol K}}}=\text{ T} \\ 72.7\text{ K = 73 K (approx.) = T} \end{gathered}`

Answer: T = 73 K