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

the answer is learned

every chemical equation adheres to the law of conservation of mass, which states that matter cannot be created or destroyed. therefore, there must be the same number of atoms of each element on each side of a chemical equation.