Please explain... a) why SO2 (g) and H2O (l) formed instead of H2 (g). I thought a metal and an acid would produce a salt and H2 (g) b) how one could predict these products. c) why CO2 (g) is formed instead of H2CO3 (aq). d) why MnO2 (s) does not participate in the reaction and how one could predict when something will be a catalyst. Are there any general rules to follow to get the right products without just memorizing every possible reaction? If I just have to memorize, could you please give me a website with information on common products to these types of reactions? [12] Write net equations for each of the reactions below. Use appropriate ionic and molecular formulas and omit formulas for all ions or molecules that do not take part in a reaction. Write structural formulas for all organic substances. You need not balance the equaon is heated strongly with a. A strip of copper metal is heated strongly with concentrated sulfuric acid. b. Solid dinitrogen pentoxide is added to water. c. Lead(II carbonate is added to hydrobromic acid. d. Freshly precipitated manganese(IV) oxide is added to a solution of hydrogen peroxide. Solution a). In the given reaction copper does not react with sulphuric acid (H2SO4), because it can not displace hydrogen form acid as it\'s reduction potential is higher than hydrogen, but here H2SO4 is an oxidising agent, redox reaction takes place so it oxidises the metal and itself reduces to SO 2 . B). nitrogen pentoxide( N2O5) is an anhydride of HNO3, it is very unstable and oxidiser. When it is reacted with H2O it can form HNO3 but in a prolonged way( slowly). the above step is part of mechanism in formation of HNO3. c)PbCO3 is a metal carboante , it is decomposed to give PbO and CO2(g), so in the given reaction CO 2 is formed. D) any compound that acst as catalyst does not partcipate in the reaction , it iniciates the reaction only.the nature of catalyst substance doesnot change during whole process of reaction. .

1. Please explain...
a) why SO2 (g) and H2O (l) formed instead of H2 (g). I thought a metal and an acid would
produce a salt and H2 (g)
b) how one could predict these products.
c) why CO2 (g) is formed instead of H2CO3 (aq).
d) why MnO2 (s) does not participate in the reaction and how one could predict when
something will be a catalyst.
Are there any general rules to follow to get the right products without just memorizing
every possible reaction? If I just have to memorize, could you please give me a website with
information on common products to these types of reactions?
[12] Write net equations for each of the reactions below. Use appropriate ionic and molecular
formulas and omit formulas for all ions or molecules that do not take part in a reaction. Write
structural formulas for all organic substances. You need not balance the equaon is heated
strongly with a. A strip of copper metal is heated strongly with concentrated sulfuric acid. b.
Solid dinitrogen pentoxide is added to water. c. Lead(II carbonate is added to hydrobromic acid.
d. Freshly precipitated manganese(IV) oxide is added to a solution of hydrogen peroxide.
Solution
a). In the given reaction copper does not react with sulphuric acid (H2SO4), because it can not
displace hydrogen form acid as it's reduction potential is higher than hydrogen, but here H2SO4
is an oxidising agent, redox reaction takes place so it oxidises the metal and itself reduces to SO 2
.
B). nitrogen pentoxide( N2O5) is an anhydride of HNO3, it is very unstable and oxidiser. When
it is reacted with H2O it can form HNO3 but in a prolonged way( slowly). the above step is part
of mechanism in formation of HNO3.
c)PbCO3 is a metal carboante , it is decomposed to give PbO and CO2(g), so in the given
reaction CO 2 is formed.

2. D) any compound that acst as catalyst does not partcipate in the reaction , it iniciates the reaction
only.the nature of catalyst substance doesnot change during whole process of reaction.