A $9.95 \cdot m o l$ $9.95mol$ quantity of ideal gas is placed in a container of $208 \cdot L$ $208L$ volume at $1.26 \cdot a t m$ $1.26*atm$ pressure. What is the temperature of the gas?

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Answer 1 · 2017-04-26T05:41:20

We can assume ideality, and find $T ≅ 320 \cdot K$ $T~=320*K$

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

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?

A 9.95*mol9.95⋅mol9.95*mol quantity of ideal gas is placed in a container of 208*L208⋅L208*L volume at 1.26*atm1.26⋅atm1.26*atm pressure. What is the temperature of the gas?