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0.24 Bis2a 06.appendix a review of red/ox reactions  (Page 7/31)

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When heated to 700–800 °C, diamonds, which are pure carbon, are oxidized by atmospheric oxygen. (They burn!) Write the balanced equation for this reaction.

C( s ) + O 2 ( g ) ⟶ CO 2 ( g )

The military has experimented with lasers that produce very intense light when fluorine combines explosively with hydrogen. What is the balanced equation for this reaction?

H 2 ( g ) + F 2 ( g ) ⟶ 2HF ( g )

Write the molecular, total ionic, and net ionic equations for the following reactions:

(a) Ca (OH) 2 ( a q ) + HC 2 H 3 O 2 ( a q ) ⟶

(b) H 3 PO 4 ( a q ) + CaCl 2 ( a q ) ⟶

(a) Ca (OH) 2 ( a q ) + 2 HC 2 H 3 O 2 ( a q ) ⟶ Ca ( C 2 H 3 O 2 ) 2 ( a q ) + 2 H 2 O( l ),
Ca 2+ ( a q ) + 2 OH − ( a q ) + 2 HC 2 H 3 O 2 ( a q ) ⟶ Ca 2+ ( a q ) + 2 C 2 H 3 O 2 − ( a q ) + 2 H 2 O( l ),
OH − ( a q ) + HC 2 H 3 O 2 ( a q ) ⟶ C 2 H 3 O 2 − ( a q ) + H 2 O( l )
(b) 2 H 3 PO 4 ( a q ) + 3 CaCl 2 ( a q ) ⟶ Ca 3 ( PO 4 ) 2 ( s ) + 6 HCl( a q ),
2 H 3 PO 4 ( a q ) + 3 Ca 2+ ( a q ) + 6 Cl − ( a q ) ⟶ Ca 3 ( PO 4 ) 2 ( s ) + 6 H + ( a q ) + 6 Cl − ( a q ),
2 H 3 PO 4 ( a q ) + 3 Ca 2+ ( a q ) ⟶ Ca 3 ( PO 4 ) 2 ( s ) + 6 H + ( a q )

Great Lakes Chemical Company produces bromine, Br 2 , from bromide salts such as NaBr, in Arkansas brine by treating the brine with chlorine gas. Write a balanced equation for the reaction of NaBr with Cl 2 .

2NaBr( a q ) + Cl 2 ( g ) ⟶ 2 NaCl( a q ) + Br 2 ( l )

In a common experiment in the general chemistry laboratory, magnesium metal is heated in air to produce MgO. MgO is a white solid, but in these experiments it often looks gray, due to small amounts of Mg 3 N 2 , a compound formed as some of the magnesium reacts with nitrogen. Write a balanced equation for each reaction.

2 Mg( s ) + O 2 ( g ) ⟶ 2 MgO( s ) ; 3 Mg( s ) + N 2 ( g ) ⟶ Mg 3 N 2 ( s )

Lithium hydroxide may be used to absorb carbon dioxide in enclosed environments, such as manned spacecraft and submarines. Write an equation for the reaction that involves 2 mol of LiOH per 1 mol of CO 2 . (Hint: Water is one of the products.)

2 LiOH( a q ) + CO 2 ( g ) ⟶ Li 2 CO 3 ( a q ) + H 2 O( l )

Calcium propionate is sometimes added to bread to retard spoilage. This compound can be prepared by the reaction of calcium carbonate, CaCO 3 , with propionic acid, C 2 H 5 CO 2 H, which has properties similar to those of acetic acid. Write the balanced equation for the formation of calcium propionate.

CaCO 3 ( s ) + 2 C 2 H 5 CO 2 H( a q ) ⟶ Ca ( C 2 H 5 CO 2 ) 2 ( a q ) + CO 2 ( g ) + H 2 O( l )

Complete and balance the equations of the following reactions, each of which could be used to remove hydrogen sulfide from natural gas:

(a) Ca ( OH ) 2 ( s ) + H 2 S( g ) ⟶

(b) Na 2 CO 3 ( a q ) + H 2 S( g ) ⟶

(a) Ca (OH) 2 ( s ) + H 2 S( g ) ⟶ CaS( s ) + 2 H 2 O( l ) ; (b) Na 2 CO 3 ( a q ) + H 2 S( g ) ⟶ Na 2 S( a q ) + CO 2 ( g ) + H 2 O( l )

Copper(II) sulfide is oxidized by molecular oxygen to produce gaseous sulfur trioxide and solid copper(II) oxide. The gaseous product then reacts with liquid water to produce liquid hydrogen sulfate as the only product. Write the two equations which represent these reactions.

CuS( s ) + 2 O 2 ( g ) ⟶ SO 2 ( g ) + CuO( s ) SO 3 ( g ) + H 2 O( l ) ⟶ H 2 SO 4 ( l )

Write balanced chemical equations for the reactions used to prepare each of the following compounds from the given starting material(s). In some cases, additional reactants may be required.

(a) solid ammonium nitrate from gaseous molecular nitrogen via a two-step process (first reduce the nitrogen to ammonia, then neutralize the ammonia with an appropriate acid)

(b) gaseous hydrogen bromide from liquid molecular bromine via a one-step redox reaction

(c) gaseous H 2 S from solid Zn and S via a two-step process (first a redox reaction between the starting materials, then reaction of the product with a strong acid)

(a) step 1: N 2 ( g ) + 3 H 2 ( g ) ⟶ 2 NH 3 ( g ), step 2: NH 3 ( g ) + HNO 3 ( a q ) ⟶ NH 4 NO 3 ( a q ) ⟶ NH 4 NO 3 ( s ) (after drying); (b) H 2 ( g ) + Br 2 ( l ) ⟶ 2 HBr( g ); (c) Zn( s ) + S( s ) ⟶ ZnS( s ) and ZnS( s ) + 2 HCl( a q ) ⟶ ZnCl 2 ( a q ) + H 2 S( g )

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Source:  OpenStax, Ucd bis2a intro to biology v1.2. OpenStax CNX. Sep 22, 2015 Download for free at https://legacy.cnx.org/content/col11890/1.1
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