Question

One of the first steps in the enrichment of uranium for use in nuclear power plants involves a displacement reaction between UO₂ and aqueous HF:

UO₂(s) + HF(aq) → UF₄(s) + H₂O(l) [unbalanced]

How many liters of 4.30 M HF will react with 4.02 kg of UO₂?


  ______L

Answer 1

we have the Balanced chemical equation as:

UO2(s) + 4 HF(aq) → UF4(s) + 2 H2O(l)

Molar mass of UO2 = 1*MM(U) + 2*MM(O)

= 1*238.0 + 2*16.0

= 270 g/mol

mass of UO2 = 4.02 Kg = 4020 g

we have below equation to be used:

number of mol of UO2,

n = mass of UO2/molar mass of UO2

=(4020 g)/(270 g/mol)

= 14.89 mol

From balanced chemical reaction, we see that

when 1 mol of UO2 reacts, 4 mol of HF reacts

mol of HF reacted = (4/1)* moles of UO2

= (4/1)*14.89

= 59.56 mol

This is number of moles of HF

we have below equation to be used:

M = number of mol / volume in L

4.3 = 59.56/ volume in L

volume = 13.9 L

Answer: 13.9 L