What volume of F2 (in liters) is required to react with 1.00 g of uranium according to the equation U(s) + 3F2(g) → UF6(g), if the temperature is 15°C and the pressure is 745 mm Hg?

Answer : The volume of required is, 0.304 L

Explanation :

First we have to calculate the moles of uranium.

Molar mass of uranium = 238.03 g/mol

Now we have to calculate the moles of

The given balanced chemical reaction is:

From the balanced chemical reaction we conclude that,

As, 1 mole of uranium react with 3 moles of

So, 0.00420 mole of uranium react with moles of

Now we have to calculate the volume of

Using ideal gas equation:

where,

P = Pressure of gas = 745 mmHg = 0.980 atm    (1 atm = 760 mmHg)

V = Volume of gas = ?

n = number of moles  = 0.0126 mole

R = Gas constant =

T = Temperature of gas =

Putting values in above equation, we get:

Thus, the volume of required is, 0.304 L

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