MCQ
The electronic configuration of silver atom in ground state is
- A$[Kr]3{d^{10}}\,4{s^1}$
- B$[Xe]\,4{f^{14}}\,5{d^{10}}\,6{s^1}$
- ✓$[Kr]\,4{d^{10}}\,5{s^1}$
- D$[Kr]\,4{d^9}\,5{s^2}$
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${A_2}\left( g \right) + {B_2}\left( g \right) \rightleftharpoons 2AB\left( g \right)$
${\Delta _r}{G^o}$ and ${\Delta _r}{S^o}$ are $20\, kJ/mol$ and $-20\, JK^{-1}\, mol^{-1}$ respectively at $200\, K$.
If ${\Delta _r}{C_P}$ is $20\, JK^{-1}\, mol^{-1}$ then ${\Delta _r}{H^o}$ at $400\, K$ is.....$kJ/mol$
$S{O_{3(g)}} \rightleftharpoons S{O_{2(g)}} + 1/2\,{O_{2(g)}}$ is $4.9 \times 10^{-2}$ then find equilibrium constant for the reaction
$2S{O_{2(g)}} + {O_{2(g)}} \rightleftharpoons 2SO_3(g)$