Titanium nitride has the formula TiN and has been used to replace gold-plating o

Question

Titanium nitride has the formula TiN and has been used to replace gold-plating on jewelry and watches. Read the entry on titanium nitride al Wikipedia and give two reasons why manufacturers would choose TiN over gold for jewelry. (One of the reasons may not be obvious from the Wiki entry.) Write the balanced equation for the formation of titanium nitride from titanium and nitrogen. "Titanium nitride" is not the correct name we would give to the produce formed in the equation in (b). What is the correct name? If you have 12.31 g of nitrogen and 20.08 g of titanium, how much titanium nitride will form? Identify the limiting reactant and the reactant in excess. How many grams of the reactant in excess will be left over if the reaction goes to completion? If you get 76.3% yield for the reaction, how many grams of titanium nitride will you recover? Titanium nitride will react with strong acids. When titanium nitride reacts with sulfuric acid, one product is ammonia. Predict the other product and balance the equation. If a reaction of titanium nitride and sulfuric acid produced 12.9 g of ammonia, how much of the second product will form? How much of each reactant was present in the reaction in part (j)? Read about titanium in The Elements. Is titanium nitride mentioned? If yes, how is it described? If no, describe two other compounds of titanium and their uses.

Explanation / Answer

a) the 2 reasons are :-

1) It has better resistance to corrosion

2) It is harder and has more varieties in color

b) 2Ti(s) + N2(g) ------> 2TiN

c) Titanium mononitride

d) Molar mass of N2 = 28 g/mole

Molar mass of Ti = 47.864 g/mole

moles of N2 in 12.31 g of it = mass/molar mass = 0.44

moles of Ti in 20.08 g of it = mas/molar mass = 20.08/47.864 = 0.42

Now, Ti and N2 reacts in the molar ratio of 2:1

Thus, Ti is the limiting reagent

Thus, moles of TiN formed = moles of Ti reacting = 0.42

Thus, mass of TiN formed = moles*molar mass = 0.42*61.864 = 25.98 g

e) Ti is the limiting reactant and N2 is in excess

f) moles of N2 left unreacted = 0.44 - 0.21 = 0.23

mass of N2 unreacted = moles*molar mass = 0.23*28 = 6.44 g

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