Question
If a mole of hydrogen molecule is heated to a high temperature then which of the following reactions take place?
A.
$${H_{2\left( g \right)}} + 436\,kJ\,mo{l^{ - 1}} \to {H_{\left( g \right)}} + {H_{\left( g \right)}}$$
B.
$$2{H_{2\left( g \right)}} + 820\,kJ\,mo{l^{ - 1}} \to 2{H_{2\left( l \right)}}$$
C.
$${H_{2\left( g \right)}} + {H_{2\left( g \right)}} + 436\,kJ\,mo{l^{ - 1}} \to $$ $$H_{\left( {aq} \right)}^ + + H_{\left( {aq} \right)}^ - $$
D.
$${H_{2\left( g \right)}} + 200\,kJ\,mo{l^{ - 1}} \to {H_{\left( g \right)}} + {H_{\left( g \right)}}$$
Answer :
$${H_{2\left( g \right)}} + 436\,kJ\,mo{l^{ - 1}} \to {H_{\left( g \right)}} + {H_{\left( g \right)}}$$
Solution :
The amount of energy required to break $$H - H$$ bond of $$1\,mole$$ of hydrogen is $$436\,kJ\,mo{l^{ - 1}}.$$
$${H_{2\left( g \right)}} + 436\,kJ\,mo{l^{ - 1}} \to {H_{\left( g \right)}} + {H_{\left( g \right)}}$$