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"Complete the equations for these single-replacement reactions in aqueous solutions. Balance each equation. Write "No reaction" if a reactions doesn't occur. Use the activity series chart you copied into your notes."

a.) Fe + Pb(NO3)2->

b.) Cl2 + NaI ->

c.) Ca + H2O ->

Verified Answer :

1.
Fe(s) + Pb(NO3)2(aq) → Fe(NO3)2(aq) + Pb(s) 

2. 
Cl2(aq) + 2 NaI(aq) → 2 NaCl(aq) + I2(aq) 

3. 
Ca(s) + 2 H2O(l) → Ca(OH)2(s) + H2(g)

Answer: a) \(Fe+Pb(NO_3)_2\rightarrow Fe(NO_3)_2+Pb\)

b.) \(Cl_2+2NaI\rightarrow 2NaCl+I_2\)

c.) \(Ca+2H_2O\rightarrow Ca(OH)_2+H_2\)

Explanation: A single replacement reaction is one in which a more reactive element displaces a less reactive element from its salt solution.

a) As iron is more reactive than lead, iron can easily lose electrons as compared to lead and result in the formation of iron nitrate and lead.

\(Fe+Pb(NO_3)_2\rightarrow Fe(NO_3)_2+Pb\)

b) As chlorine is more reactive than iodine , chlorine can easily replace iodine from its salt solution and result in the formation of sodium chloride and iodine.

\(Cl_2+2NaI\rightarrow 2NaCl+I_2\)

c) As calcium is more reactive than hydrogen, calcium can easily lose electrons as compared to hydrogen and result in the formation of  calcium hydroxide and hydrogen.

\(Ca+2H_2O\rightarrow Ca(OH)_2+H_2\)

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