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Chapter 4: Q4.56P (page 180)

One of the first steps in the enrichment of uranium for use in nuclear power plants involves a displacement reaction between ${UO}_{2} ?$ and aqueous HF:
${UO}_{2} (s) + HF (aq) 鈫� {UF}_{4} (s) + H_{2} O (l) (unbalanced)$
How many liters of 2.40 M HF will react with 2.15 kg of ${UO}_{2} ?$

Short Answer

Expert verified

13.27 lit liters of 2.40 M HF will react with 2.15 kg of ${UO}_{2}$ .

Step by step solution

01

Write down the balanced molecular equation

The reaction is shown below.

${UO}_{2} (s) + 4 HF (aq) 鈫� {UF}_{4} (s) + 2 H_{2} O (l)$

02

Calculate the moles of HF

Given values are:

The mass of = 2.15 kg and the molarity of HF = 2.40 M

Moles of HFare:

$\begin{matrix} {苍耻尘产别谤鈥塷蹿鈥尘辞濒别蝉鈥塷蹿鈥塙翱}_{2} = \frac{2.15鈥嬧赌塳驳脳1000鈥塯}{270.03} \\ = 7.96 鈥尘辞濒别蝉 \end{matrix}$

One mole of ${UO}_{2}$ react with 4 moles of HF. Therefore,

尘辞濒别鈥夆赌塺补迟颈辞鈥�=鈥� \frac{4鈥夆€尘辞濒别蝉鈥夆€塇F}{{1鈥夆赌尘辞濒别鲍翱}_{2}} = 4

Number of moles of HF that reacted with $7.96 鈥尘辞濒别蝉$ of ${UO}_{2}$ is calculated below.

$Number鈥塷f鈥尘辞濒别蝉of鈥塇F = 7.96 脳 4 = 31.85$

03

Calculate the volume of HF

The volume of HF to react completely with 2.15 kg of ${UO}_{2}$

role="math" localid="1658752947679" $\begin{matrix} volume of HF & = & \frac{moles of HF}{molarity of HF} \\ = & \frac{31.85 molHF}{(\frac{2.40 molHF}{1 litHF})} \\ = 13.27 literHF \end{matrix}$

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Most popular questions from this chapter

$8 N H_{3} (g) + 6 N O_{2} (g) 鈫� 7 N_{2} (g) + 12 H_{2} O (l)$ Identify the oxidizing agent and the reducing agent in the following reaction, and explain your answer:

Thyroxine (C₁₅H₁₁I₄NO₄) is a hormone synthesized by the thyroid gland and used to control many metabolic functions in the body. A physiologist determines the mass percent of thyroxine in a thyroid extract by igniting 0.4332 g of extract with sodium carbonate, which converts the iodine to iodide. The iodide is dissolved in water, and bromine and hydrochloric acid are added, which convert the iodide to iodate.

(a) How many moles of iodate form per mole of thyroxine?

(b) Excess bromine is boiled off and more iodide is added, which reacts as shown in the following unbalancedequation:

${IO}_{3}^{-} (aq) + H^{+} (aq) + I^{-} (aq) 鈫� I_{2} (aq) + H_{2} O (I)$

How many moles of iodine are produced per mole of thyroxine?

(Hint:Be sure to balance the charges as well as the atoms.) What are the oxidizing and reducing agents in the reaction?

(c) The iodine reacts completely with 17.23 mL of 0.1000 Mthiosulfate as shown in the following unbalancedequation:

$I_{2} (aq) + S_{2} O_{3}^{2 -} (aq) 鈫� I^{-} (aq) + S_{4} O_{6}^{2 -} (aq)$

What is the mass percent of thyroxine in the thyroid extract?

You are given solutions of HCl and NaOH and must determine their concentrations. You use 27.5mL of NaOH to titrate 100mL of HCl and 18.4mL of NaOH to titrate 50.0mL of 0.0782M H₂SO₄. Find the unknown concentrations.

Predict the product(s) and write a balanced equation for each of the following redox reactions:

$(a) M g (s) + H C l (a q) 鈫�$

$(b) L i C l (l) \overset{eletricity}{鈫�}$ $(b) L i C l (l) \overset{e l e t r i c i t y}{鈫�}$

$(c) S n C l_{2} (a q) + C o (s) 鈫�$

The net ionic equation for the aqueous neutralization reaction between acetic acid and sodium hydroxide is different from that for the reaction between hydrochloric acid and sodium hydroxide. Explain by writing balanced net ionic equations.

See all solutions

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