Question

What is the pressure in atm of a 2.00 mole sample of H2 in 5.00 L flask at 65oC? Report answer to nearest tenth.

Answer 1

`11.1\text{ atm}`

Step-by-step explanation:

Here, we want to get the pressure in atm

We can use the ideal gas formula to get this

Mathematically:

`PV\text{ = nRT}`

P is the pressure in atm which we want to calculate

V is the volume which is given as 5 L

n is the number of moles which is 2 moles

T is the temperature (we have to convert this to Kelvin by adding 273.15 K : 273.15 + 65 = 338.15 K)

R is the molar gas constant which is 0.0821 Latm/mol.K

Substituting the values, we have it that:

`\begin{gathered} P\text{ = }(nRT)/(V) \\ \\ P\text{ = }(2*0.0821*338.15)/(5)\text{ = 11.1 atm} \end{gathered}`