Exercise 1 .- Convert these descriptions into balanced chemical equations: • Whe

Question

Exercise 1
.- Convert these descriptions into balanced chemical equations:

• When the sulfur trioxide gas reacts with water, a solution of sulfuric acid

• Metallic copper reacts with a hot concentrated solution of sulfuric acid to form aqueous copper (II) sulfate, gaseous sulfur dioxide and water.

• Heating solid mercury (II) nitrite decomposes to form solid mercury (II) oxide, gaseous nitrogen dioxide and oxygen.

• Silver nitrite reacts with sodium sulfate to produce silver sulfate and sodium nitrite.

• Solid ammonium nitrite has a decomposition reaction giving nitrogen and oxygen gas and water vapor as products.

Exercise 2.
Mandelic acid is an organic acid formed of Carbon (63.15%), Hydrogen (5.30%), and
Oxygen (31.55%).
Its molar mass is 152.14 grs./mol.
Calculate the empirical and molecular formula

Exercise 3
Some coal contains 2.5% by mass of sulfur. When this coal is burned, the sulfur is converted to gaseous sulfur dioxide. The sulfur dioxide is reacted with calcium oxide to form solid calcium sulfite.
a.- Write the balanced equation for the reaction.
b.- If the coal is burned in an energy plant that spends 2000 tons of coal a day, calculate the daily production of calcium sulphite.

Exercise 4.
In the laboratory there are two solutions which, when mixed, produce a chemical reaction. Calculate the grams in the before and after reaction. In the table write down the chemical names of the reagents and products.
Dissolution 1. 200 milliliters of 6N Iron Hydroxide solution.
Dissolution 2. 300 milliliters of 3N Sulfuric Acid.
Reaction.

2Fe(OH)3 (ac)        +           3 H2SO4 (ac)           Fe2(SO4)3 (ac)       +        6H2O

Exercise 5.
In the laboratory there are two solutions which, when mixed, produce a chemical reaction. Calculate the grams in the before and after reaction. In the table write down the chemical names of the reagents and products.
Dissolution 1. 200 milliliters of 7N Sodium Carbonate solution.
Dissolution 2. 500 milliliters of 2M hydrochloric acid at 35% by mass.
Reaction.

Na2CO3 (ac)        +           2 HCl (ac)         2NaCl       +     H2CO3 (ac)

Exercise 6.
In the laboratory there are two solutions which, when mixed, produce a chemical reaction. Calculate the grams in the before and after reaction. In the table write down the chemical names of the reagents and products.
Dissolution of iron oxide III at 8 m, containing 200 milliliters of water. It is mixed with 25 grams of carbon monoxide.
Reaction.

Fe2O3(ac)        +           3 CO (g)          2 Fe (s)       +       3CO2

Exercise 7.
Calcium carbonate reacts with a solution of hydrochloric acid to form a solution of calcium chloride, water and carbon dioxide
What is the percentage yield of carbon dioxide if 3.65 grams of the gas is collected when 10 grams of calcium carbonate is reacted?

HCl (ac)       +       CaCO3(s)                            CaCl2(ac)      +    H2O (l)    + CO2(g)

Exercise 8.
Titanium is a strong, lightweight and corrosion resistant metal used in the construction of spacecraft, aircraft, aircraft engines and bicycle frames. It is obtained by the reaction of Titanium chloride IV with molten magnesium between 950 and 1150 C

Reaction:
TiCl4 (g) + 2 Mg (l)                Ti (s) + 2MgCl 2 (l)

In a certain industrial operation, 3.54 x 10 7 grams of TiCl 4 are reacted with 1.13 × 10 7 grams of magnesium. Calculate the percentage of yield if in fact you get 7.91 x 106 grams of Ti

Explanation / Answer

Ans 1 :

The reactions are framed according to the chemical processes mentioned. Then the atoms on the both sides are balanced .

The balanced reactions are :

SO3 (g) + H2O (l)= H2SO4 (aq)

Cu (s) + 2H2SO4 (aq)= CuSO4 (aq) + SO2 (g)+ 2H2O (l)

2Hg(NO2)2 (s) = HgO (s) + 4NO2 (g) + -1O2 (g)

2AgNO3 + Na2SO4 = Ag2SO4 + 2NaNO3

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