91Ó°ÊÓ

Which is a decomposition reaction and which is not? a) \(3 \mathrm{O}_{2} \rightarrow 2 \mathrm{O}_{3}\) b) \(2 \mathrm{KClO}_{3} \rightarrow 2 \mathrm{KCl}+3 \mathrm{O}_{2}\)

In the reaction $$ 2 \mathrm{Ni}(\mathrm{s})+3 \mathrm{I}_{2}(\mathrm{~s}) \rightarrow 2 \mathrm{NiI}_{3}(\mathrm{~s}) $$ indicate what has been oxidized and what has been reduced.

What are two different definitions of oxidation?

Which is a decomposition reaction and which is not? a) \(\mathrm{Na}_{2} \mathrm{O}+\mathrm{CO}_{2} \rightarrow \mathrm{Na}_{2} \mathrm{CO}_{3}\) b) \(\mathrm{H}_{2} \mathrm{SO}_{3} \rightarrow \mathrm{H}_{2} \mathrm{O}+\mathrm{SO}_{2}\)

Write a balanced chemical equation for the neutralization reaction between each given acid and base. Include the proper phase labels. a) \(\mathrm{HI}(\mathrm{aq})+\mathrm{KOH}(\mathrm{aq}) \rightarrow ?\) b) \(\mathrm{H}_{2} \mathrm{SO}_{4}(\mathrm{aq})+\mathrm{Ba}(\mathrm{OH}) 2(\mathrm{aq}) \rightarrow ?\)

Write the complete ionic equation for the reaction of \(\mathrm{Fe}_{2}\left(\mathrm{SO}_{4}\right)_{3}(\mathrm{aq})\) and \(\mathrm{Sr}\left(\mathrm{NO}_{3}\right)_{2}(\mathrm{aq})\). You may have to consult the solubility rules.

Write a balanced chemical equation for the neutralization reaction between each given acid and base. Include the proper phase labels. a) \(\mathrm{HNO}_{3}(\mathrm{aq})+\mathrm{Fe}(\mathrm{OH})_{3}(\mathrm{~s}) \rightarrow ?\) b) \(\mathrm{H}_{3} \mathrm{PO}_{4}(\mathrm{aq})+\mathrm{CsOH}(\mathrm{aq}) \rightarrow ?\)

Which is a decomposition reaction and which is not? a) \(2 \mathrm{C}_{7} \mathrm{H}_{5} \mathrm{~N}_{3} \mathrm{O}_{6} \rightarrow 3 \mathrm{~N}_{2}+5 \mathrm{H}_{2} \mathrm{O}+7 \mathrm{CO}+7 \mathrm{C}\) b) \(\mathrm{C}_{6} \mathrm{H}_{12} \mathrm{O}_{6}+6 \mathrm{O}_{2} \rightarrow 6 \mathrm{CO}_{2}+6 \mathrm{H}_{2} \mathrm{O}\)

Use the periodic table or the activity series to predict if each single- replacement reaction will occur and, if so, write a balanced chemical equation. a) \(\mathrm{Zn}+\mathrm{Fe}_{3}\left(\mathrm{PO}_{4}\right)_{2} \rightarrow\) ? b) \(\mathrm{Ag}+\mathrm{HNO}_{3} \rightarrow ?\)

Assign oxidation numbers to each atom in each substance. a) \(\mathrm{P}_{4}\) b) \(\mathrm{SO}_{2}\) c) \(\mathrm{SO}_{2}^{2-}\) d) \(\mathrm{Ca}\left(\mathrm{NO}_{3}\right)_{2}\)