Question

A `9.95*mol` quantity of ideal gas is placed in a container of `208*L` volume at `1.26*atm` pressure. What is the temperature of the gas?

Answer 1

We can assume ideality, and find `T~=320*K`

Explanation:

`T=(PV)/(nR)= (1.26*cancel(atm)xx208*cancelL)/(9.95*cancel(mol)xx0.0821*cancel(L*atm)*K^-1*cancel(mol^-1))`

At least this is dimensionally consistent. We wanted an answer in `K`, we got an answer in `1/(K^-1)=1/(1/K)=K` as required............

So two questions:

From where did I get the expression `T=(PV)/(nR)`?

If we had measured `"ammonia gas"` or `"hydrogen chloride"` would our assumption of ideality be justified?