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Charra [1.4K]
3 years ago
6

Chlorine gas is added to a large flask to a pressure of 1.85 atm, at a temperature of 322 K. Phosphorus is added, and a reaction

takes place using all of the Cl2 gas. When the reaction is complete, the yield of PCl5 is measured at 118 grams. Calculate the Volume of the flask (in Liters): g
Chemistry
1 answer:
AVprozaik [17]3 years ago
8 0

Answer:

The volume of the flask is<u> 20.245 litres .</u>

Explanation:

We are given with following information-

PV=nRT -------- 1

where R =0.0821L.atom/mole.K

Molar mass of PCl_5=208.22g/mole

The given chemical equation is -

2P _(_s_)+5Cl_2 _(_g_)\rightarrow2PCl_5  _(_s_) --------- 2

Now , calculation -

Mass of PCl_5 formed = 118g

Molar mass of PCl_5 = 208.22g/mole

      Mole = \frac{mass (g)}{molar mass}

Therefore , moles of PCl_5 formed = \frac{118}{208.22}

     From equation 2 , we get to know that ,

 2mole PCl_5 formed from 5 mole Cl_2 _(_g_)

Therefore , \frac{118}{208.22} mole PCl_5 formed from \frac{5}{2} \times\frac{118}{208.22} mole Cl_2 _(_g_)

Moles of Cl_2 _(_g_) used =\frac{5\times118}{2\times208.22} mole

R= 0.0821L.atom/mole.K

Pressure (P)= 1.85atm

Temperature (T)= 322K

Moles of  Cl_2 _(_g_) (n)= \frac{5}{2} \times\frac{118}{208.22} moles

Applying  the formula above in 1 equation , that is

PV = nRT

putting the given values -

1.85 \times V=\frac{5}{2} \times\frac{118}{208.22}\times0.0821\times322

 V = 20.245 litres.

Hence , the volume of the flask is <u>20.245 litres . </u>

 

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