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answer questions homework
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CHEM 110 Homework 4
Name ________________ Student ID ______________ Date ______________
1
How many moles of oxygen can be obtained by the decomposition of 7.5 mol of
reactant in each of the following reactions?
5 points
(a) 2 KClO3 → 2 KCl + 3 O2
(b) 2 H2O2 → 2 H2O + O2
(c) 2 HgO → 2 Hg + O2
(d) 2 NaNO3 → 2 NaNO2 + O2
(e) KClO4 → KCl + 2 O2
2
In petroleum refining, hydrocarbons are often manipulated by reacting them with
H2(g). If hexene, C6H12 is reacted with hydrogen to form hexane, C6H14, how many moles
of hydrogen are needed to react with 453 moles of hexene?
5 points
3
The combustion of liquid chloroethylene, C2H3Cl, yields carbon dioxide, steam,
and hydrogen chloride gas. (a) Write a balanced equation for the reaction. (b)
How many moles of oxygen are required to react with 35.00 g of
chloroethylene? (c) If 25.00 g of chloroethylene reacts with an excess of
oxygen, how many grams of each product are formed?
10 points
4
A gas is known to be either CH4 or C2H6. A 1.00-g sample of this gas produces
1.80 g of water when combusted in excess O2. Assuming complete combustion to CO2
and H2O, which gas is it?
10 points
5
The equation for one of the reactions in the process of turning iron ore into the
metal is Fe2O3(s) + 3 CO(g) → 2 Fe(s) + 3 CO2(g)
If you start with 2.00 kg of each reactant, what is the maximum mass of iron you
can produce?
10 points
6
Hydrogen and oxygen are reacted and the water formed is collected at 25°C,
where it has a density of 0.997 g/mL. If 36.8 g of H2 and 168 g of O2 are reacted, how
many mL of water will be collected?
10 points
7
.
When iron and steam react at high temperatures, the following reaction takes
place: 3 Fe(s) + 4 H2O(g) → Fe3O4(s) + 4 H2(g)
How much iron must react with excess steam to form 897 g of Fe3O4 if the
reaction yield is 69%?
10 points
8
Sulfur hexafluoride is a very stable gas useful in electrical generators and
switches. It is formed by direct synthesis from the elements.
S(s) + 3 F2(g) → SF6(g)
If 92 g of SF6 is produced from the reaction of 115 g of sulfur in excess fluorine,
what is the percentage yield?
10 points
9
A mixture of 10.0 g of NO and 14.0 g of NO2 results in the production of 8.52 g
of N2O3. What is the percentage yield?
10 points
NO(g) + NO2(g) → N2O3()
10
A metallurgical firm needs to dispose of 2.74 103 gallons of waste
sulfuric acid whose concentration has been determined to be 1.53 M.
Environmental regulations require them to neutralize the waste before
releasing the waste water, and they choose to do so with slaked lime,
Ca(OH)2(s). The neutralization reaction is:
H2SO4(aq) + Ca(OH)2(s) → CaSO4(s) + 2 H2O()
If the slaked lime costs $0.52 per pound, how much will it cost to
neutralize the waste sulfuric acid?
10 points
11
Elemental analysis is sometimes carried out by combustion of the sample. For a
hydrocarbon, the only products formed are CO2 and H2O. If a 1.36-g sample of
an unknown hydrocarbon is burned and 2.21 g of H2O are produced along with
4.07 g of CO2, what is the empirical formula of the hydrocarbon?
10 points
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