At what temperature will 5.00 g of $C l_{2}$ $Cl_2$ exert a pressure of 900. mmHg at a volume of 750. ml?

Question

13937 views around the world

You can reuse this answer
Creative Commons License

Answer 1 · 2018-05-12T18:26:54

Given,

$n = 5.00 g \cdot \frac{mol}{71 g} \approx 7.04 \cdot 10^{- 2} mol$ $n = 5.00"g" * "mol"/(71"g") approx 7.04*10^-2"mol"$

$V = 0.750 L$ $V = 0.750"L"$

$P = 900 mmHg \cdot \frac{atm}{760 mmHg} \approx 1.18 atm$ $P = 900"mmHg" * "atm"/(760"mmHg") approx 1.18"atm"$

Recall,

$P V = n R T$ $PV = nRT$

Hence,

$=>T = (PV)/(nR) approx 154°"C"$

is the temperature at which this gas will behave in accordance with those parameters, given ideal behavior.

At what temperature will 5.00 g of Cl_2Cl2Cl_2 exert a pressure of 900. mmHg at a volume of 750. ml?