4. What is the density of UF6 at 100°C and 1 atm? It is a very dense gas. 5. Ele

Question

4. What is the density of UF6 at 100°C and 1 atm? It is a very dense gas.

5. Elemental sulfur can be recovered from gaseous hydrogen sulfide through the reaction:

2 H2S (g) + SO2 (g) ® 3 S (s) + 2 H2O (l)

What volume of H2S (in L, at 0.00°C and one atm) is required to produce 2.00 kg of sulfur by this

process?

6. Sulfur dioxide reacts with oxygen to give sulfur trioxide. Suppose that at one stage of the reaction

26.0 mol SO2, 83.0 mol O2, and 17.0 mol SO3 are present in the reaction vessel, and the total

pressure of the system is 0.950 atm. Calculate the mole fraction of SO3 and its partial pressure.

7. The following arrangement of flasks is set up. Assuming no temperature change and no reaction,

determine (a) the final pressure inside the system after all stopcocks are opened and (b) the mole

fraction of each gas. Assume that the connecting tube has no volume.

l________________________l______________________________l

O2(g)                                    N2(g)                                                    Ar (g)

V= 5.00 L                             V= 4.00 L                                             V=3.00 L

P= 2.51 atm                         P=0.792 atm                                        P= 1.23atm

Explanation / Answer

4)
P = 1.0atm
T= 100.0 oC
= (100.0+273) K
= 373 K

Molar mass of UF6,
MM = 1*MM(U) + 6*MM(F)
= 1*238.0 + 6*19.0
= 352 g/mol

Lets derive the equation to be used
use:
p*V=n*R*T
p*V=(mass/molar mass)*R*T
p*molar mass=(mass/V)*R*T
p*molar mass=density*R*T

Put Values:
1.0 atm *352.0 g/mol = density * 0.0821 atm.L/mol.K *373.0 K
density = 11.5 g/L
Answer: 11.5 g/L

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