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Chapter 4: Q4.63P (page 180)

8NH3(g)+6NO2(g)鈫�7N2(g)+12H2O(l)Identify the oxidizing agent and the reducing agent in the following reaction, and explain your answer:

Short Answer

Expert verified

Answer: You need to identify the oxidizing agent and reducing agent of the given reaction.

Step by step solution

01

Oxidation state of nitrogen in NH3 

Oxidation state of Hydrogen attached to non-metal is +1.

Let, oxidation state of nitrogen in NH3 is x.

No you can write,

x+3+1=0x=-3

02

Oxidation state of nitrogen in NO2 

Oxidation state of Oxygen attached to non-metal is -2.

Let, oxidation state of nitrogen in NO2 is y.

No you can write,

y+2-2=0y=+4

03

Oxidation state of nitrogen in N2 

Oxidation state of nitrogen in N2 is 0.

04

Conclusion

In the given reaction

8NH3g+6NO2g鈫�7N2g+12H2Ol

The oxidation state of nitrogen in NH3 is -3 which increases to 0 in N2. Therefore, NH3 undergoes oxidation in this given reaction. Hence, it acts as a reducing agent.

The oxidation state of nitrogen in NO2 is +4 which reduces to 0 in N2. Therefore, NO2 undergoes reduction in this given reaction. Hence, it acts as an oxidizing agent.

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Most popular questions from this chapter

Why must every redox reaction involve an oxidizing agent and a reducing agent?

Calcium dihydrogen phosphate, Ca(H2PO4)2, and sodium hydrogen carbonate, NaHCO3, are ingredients of baking powder that react with each other to produce CO2, which causes dough or batter to rise:

Ca(H2PO4)2(s)+NaHCO3(s)鈫�CO2(g)+H2O(g)+CaHPO4(s)+Na2HPO4(s)

[unbalanced]

If the baking powder contains 31% NaHCO3and 35% Ca(H2PO4)2 by mass:

(a) How many moles of CO2 are produced from 1.00 g of baking powder?

(b) If 1 mol of CO2 occupies 37.0 L at 350_F (a typical baking temperature), what volume of CO2is produced from 1.00 g of baking powder?

(a) Name three common strong acids.

(b) Name three common strong bases.

(c) What is a characteristic behavior of a strong acid or a strong base?

For the following aqueous reactions, complete and balance the molecular equation and write a net ionic equation:

(a) Manganese(II) sulfide + hydrobromic acid

(b) Potassium carbonate + strontium nitrate

(c) Potassium nitrite + hydrochloric acid

(d) Calcium hydroxide + nitric acid

(e) Barium acetate + iron(II) sulfate

(f) Zinc carbonate + sulfuric acid

(g) Copper(II) nitrate + hydrosulfuric acid

(h) Magnesium hydroxide + chloric acid

(i) Potassium chloride + ammonium phosphate

(j) Barium hydroxide + hydrocyanic acid

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:

IO3-(aq)+H+(aq)+I-(aq)鈫�I2(aq)+H2O(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:

I2(aq)+S2O32-(aq)鈫�I-(aq)+S4O62-(aq)

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