- A$1{s^2}2{s^2}2{p^6}3{s^2}3{p^6}3{d^5}$
- B$1{s^2}2{s^2}2{p^6}3{s^2}3{p^6}4{s^2}3{d^5}$
- C$1{s^2}2{s^2}2{p^6}3{s^2}3{p^6}4{s^2}3{d^7}$
- ✓$1{s^2}2{s^2}2{p^6}3{s^2}3{p^6}4{s^2}3{d^6}$
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$C _{2} H _{6} \rightarrow C _{2} H _{4}+ H _{2}$
the reaction enthalpy $\Delta_{ r } H =...........{ kJ\, mol ^{-1}}$.
(Round off to the Nearest Integer).
[Given : Bond enthalpies in $kJ$ $mol$ $^{-1}:C-C : 347, C = C : 611 ; C - H : 414, H - H : 436]$
$n = 3, l = 1, m_l = 0$
Statement $I:$ Upon heating a borax bead dipped in cupric sulphate in a luminous flame, the colour of the bead becomes green.
Statement $II:$ The green colour observed is due to the formation of copper(I) metaborate.
In the light of the above statements, choose the most appropriate answer from the options given below :
$X \rightleftharpoons 2Y$ and $Z \rightleftharpoons P + Q,$
respectively are in the ratio of $1 : 4.$ If the degree of dissociation of $X$ is $2$ times that of $Z,$ then the ratio of total pressure $(P_1 : P_2)$ at these equilibria is : (Assume degree of dissociation for both reactions are very very small)
$\left[\mathrm{TeBr}_6\right]^{2-},\left[\mathrm{BrF}_2\right]^{+}, \mathrm{SNF}_3 \text {, and }\left[\mathrm{XeF}_3\right]^{-}$ (Atomic numbers : $\mathrm{N}=7, \mathrm{~F}=9, \mathrm{~S}=16, \mathrm{Br}=35, \mathrm{Te}=52, \mathrm{Xe}=54$ )
$NO(g) \rightarrow \frac{1}{2} N_2(g)+ \frac{1}{2} O_2(g)$ at the same temperature is :