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Solve it, The equation which is balanced and represents the correct product(s) is :

  The equation which is balanced and represents the correct product(s) is :

  • Option 1)

    Li_{2}O+2KCl\rightarrow 2LiCl+K_{2}O

  • Option 2)

    \left [ CoCl\left ( NH_{3} \right )_{5} \right ]^{+}+5H^{+}\rightarrow Co^{2+}+5NH_{4}^{+}+Cl^{-}

  • Option 3)

    \left [ Mg\left ( H_{2}O \right )_{6} \right ]^{2+}+(EDTA)^{4-}\xrightarrow[]{excess NaOH}\left [ Mg(EDTA) \right ]^{2+}+6H_{2}O

  • Option 4)

    CuSO_{4}+4KCN\rightarrow K_{2}\left [ Cu(CN)_{4} \right ]+K_{2}SO_{4}

 
Answers (1)
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As we learned

 

Oxides and hydroxides of Li and Mg -

1. They are much less soluble

2. Their hydroxides decomposes on heating

3. Their oxides don't combine with excess oxygen to give superoxide

-

 

 In Li_{2}O+2KCl\rightarrow 2LiCl+K_{2}O

This reaction is unfavourable in forward direction as Li2O is more stable than K2O . In eqn 3 charge on \left [ Mg\left ( E\: DT\: A \right ) \right ] should be -2 inspite of +2.

In eqn 4, product should be K_{3}\left [ Cu\left ( CN \right )_{4} \right ] .

Only, \left [ CoCl\left ( NH_{3} \right )_{5} \right ]^{+}+5H^{+}\rightarrow CO^{2+}+5NH_{4}^{+}+Cl^{-}  is balanced and represents correct products.


Option 1)

Li_{2}O+2KCl\rightarrow 2LiCl+K_{2}O

Option 2)

\left [ CoCl\left ( NH_{3} \right )_{5} \right ]^{+}+5H^{+}\rightarrow Co^{2+}+5NH_{4}^{+}+Cl^{-}

Option 3)

\left [ Mg\left ( H_{2}O \right )_{6} \right ]^{2+}+(EDTA)^{4-}\xrightarrow[]{excess NaOH}\left [ Mg(EDTA) \right ]^{2+}+6H_{2}O

Option 4)

CuSO_{4}+4KCN\rightarrow K_{2}\left [ Cu(CN)_{4} \right ]+K_{2}SO_{4}

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