question archive Choose a binary ionic compound, demonstrate a balanced chemical equation for decomposition of this compound
Choose a binary ionic compound, demonstrate a balanced chemical equation for decomposition of this compound
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Choose a binary ionic compound, demonstrate a balanced chemical equation for decomposition of this compound. Based on 1.0 gram of your compound, give the masses of each element after decomposition has occurred. How does this data verify the Law of Conservation of Matter?
12. Consider only synthesis and decomposition reactions. Describe 3 ways you could synthesize a group 2 metal oxide.
13. A student reacted metals A, B, C and D with metal salts AX, BX, CX and DX and obtained the following data.
Reacting Species
AX
BX
CX
DX
A
---
Reaction
No Reaction
Reaction
B
No Reaction
---
Reaction
Reaction
C
Reaction
Reaction
---
Reaction
D
No Reaction
No Reaction
No Reaction
---
Provide an activity series (ranked with the most active metals at the bottom) for the metals A, B, C, and D based on the data in the table.
14. Copper(I) nitrate (CuNO3 (aq)) reacts with potassium phosphate (K3PO4(aq)) and a precipitate is formed.
a) Indicate the type of reaction.
b) Write the balanced chemical equation and indicate which substance forms the precipitate.
15. Vanadium(IV) nitrate (V(NO3)4 (aq)) reacts with sodium carbonate (Na2CO3(aq)) and a precipitate is formed.
a) Indicate the type of reaction.
b) Write the balanced chemical equation and indicate which substance forms the precipitate.
16. Sulfuric acid (H2SO4) reacts with sodium bicarbonate (NaHCO3).
a) Indicate the type of reaction.
b) Write the balanced chemical equation.
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Consider decomposition of Iron(III)Chloride compound when heated above 500oC. This ionic compound decomposes into Iron(II)Chloride and carbon dioxide as shown by the equation below.
2FeCl3(s) + Heat => 2 FeCl2(s) + Cl2(g)
Decomposing 1.0 gram FeCl3 of gives 0.4 grams FeCl2 and 0.6 grams Cl2 hence obeying the law of mass conservation.
12)Example of group 2 metal is magnesium and its oxide is magnesium oxide. Below are synthetic and decomposition reactions that form magnesium oxide.
a) Decomposition of Magnesium carbonate.
Heating magnesium carbonate in a furnace at temperature of 350oC, magnesium carbonate decompose into magnesium oxide and carbon dioxide as illustrated in the reaction below.
MgCO3(s) + Heat => MgO(s) + CO2(g)
b) Oxidation of metal Magnesium metal in oxygen
Burn a metal magnesium in oxygen rich condition to obtain metal oxide of magnesium as illustrated in the reaction below.
2Mg(s) +O2(s) => 2MgO(s)
c)Decomposition of magnesium nitrate
Heating magnesium nitrate in temperature of 160oC results to decomposition of the metal nitrate to form metal oxide, nitrogen dioxide and oxygen gases.
2Mg(NO3)2(s) + Heat => 2MgO(s) + 4 NO2(g) + O2(g)
13) C>A>B>D.
14) a) Displacement reaction.
b)3Cu(NO3)2(aq) + 2K3PO4(aq) => 6KNO3(aq) + (Cu)3(PO4)2(s)
(Cu)3(PO4)2(aq) forms the precipitate.
15)a) Displacement reaction.
b) 2V(NO3)4(aq) + 4 Na2CO3(aq) => V2(CO3)4(s) + 8 NaNO3(aq)
V2(CO3)4(s) forms the precipitate.
16)a) Decomposition reaction.
b) H2SO4(aq) + 2NaHCO3(aq) => Na2SO4(aq) + 2 CO2(g) + 2H2O(l)
12) Group 2 metal oxides are formed through different synthetic methods including oxidation with oxygen, displacement of oxides of metals lower in the reactivity series and decomposition reactions. Group two metals are strongly reactive forming stable oxide which is not easily reduced or decomposed further.
13) C is most reactive since its salt cannot be displaced by either A,B, or D. A is the second most reactive since its salt cannot be displaced by by either B or D. B is the third most reactive since its salt cannot be displaced by D. D is the least reactive since it cannot displace all the other salts.
14)a)Displacement reactions involve taking of ions from the least reactive metal by the most reactive element hence displacing the ions from the least reactive metal.
b) All nitrates of group one are soluble hence potassium nitrate forms no precipitates. Phosphates of transition metals are insoluble hence copper phosphate forms precipitate.
15) a)Displacement reactions involve taking of ions from the least reactive metal by the most reactive element hence displacing the ions from the least reactive metal as expressed by the reaction of vanadium(IV)nitrate and sodium carbonate.
b) Transition metal carbonates are insoluble while nitrates of group one are soluble hence precipitate of vanadium carbonate is formed.
16) a)Decomposition reactions results into breaking the compound too its simplest constituents.
b) The reaction of sulfuric acid with bicarbonate is a decomposition reaction in which sodium sulfate is formed in addition to carbon dioxide, and water.
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