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					4.59 Which type of redox reaction leads to the following?
(a) An increase in the number of substances
(b) A decrease in the number of substances
(c) No change in the number of substances




4.60 Why do decomposition reactions typically have
compounds as reactants, whereas combination and
displacement reactions have one or more elements?




4.61 Which of the three types of reactions discussed in this
section commonly produce one or more compounds?
4.62 Balance each of the following redox reactions and classify
it as a combination, decomposition, or displacement reaction:
(a) Sb(s) + Cl2(g)  SbCl3(s)


(b) AsH3(g)  As(s) + H2(g)


(c) Mn(s) + Fe(NO3)3(aq)  Mn(NO3)2(aq) + Fe(s)
4.63 Balance each of the following redox reactions and classify
it as a combination, decomposition, or displacement reaction:
(a) Mg(s) + H2O(g)  Mg(OH)2(s) + H2(g)


(b) Cr(NO3)3(aq) + Al(s)  Al(NO3)3(aq) + Cr(s)


(c) PF3(g) + F2(g)  PF5(g)




4.64 Predict the product(s) and write a balanced equation for
each of the following redox reactions:
(a) N2(g) + H2(g) 




(c) Ba(s) + H2O(l) 
4.65 Predict the product(s) and write a balanced equation for
each of the following redox reactions:
(a) Fe(s) + HClO4(aq) 


(b) S8(s) + O2(g) 


4.66 Predict the product(s) and write a balanced equation for
each of the following redox reactions:
(a) Cesium + iodine 


(b) Aluminum + aqueous manganese(II) sulfate 


(c) Sulfur dioxide + oxygen 


(d) Propane and oxygen 


(e) Write a balanced net ionic equation for (b).
4.67 Predict the product(s) and write a balanced equation for
each of the following redox reactions:
(a) Pentane (C5H12) + oxygen 


(b) Phosphorus trichloride + chlorine 


(c) Zinc + hydrobromic acid 


(d) Aqueous potassium iodide + bromine 


(e) Write a balanced net ionic equation for (d).


4.68 How many grams of O2 can be prepared from the thermal
decomposition of 4.27 kg of HgO? Name and calculate the mass
(in kg) of the other product.
4.69 How many grams of chlorine gas can be produced from
the electrolytic decomposition of 874 g of calcium chloride?
Name and calculate the mass (in g) of the other product.




4.70 In a combination reaction, 1.62 g of lithium is mixed with
6.00 g of oxygen. (a) Which reactant is present in excess? (b)
How many moles of product are formed? (c) After reaction,
how many grams of each reactant and product are present?
4.71 In a combination reaction, 2.22 g of magnesium is heated
with 3.75 g of nitrogen. (a) Which reactant is present in excess?
(b) How many moles of product are formed? (c) After reaction,
how many grams of each reactant and product are present?




4.72 A mixture of CaCO3 and CaO weighing 0.693 g was heated
to produce gaseous CO2. After heating, the remaining solid
weighed 0.508 g. Assuming all the CaCO3 broke down to CaO
and CO2, calculate the mass percent of CaCO3 in the original
mixture.
4.73 Before arc welding was developed, a displacement
reaction involving aluminum and iron(III) oxide was commonly
used to produce molten iron (the thermite process). This
reaction was used, for example, to connect sections of iron
railroad track. Calculate the mass of molten iron produced
when 1.00 kg of aluminum reacts with 2.00 mol of iron(III)
oxide.

				
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