Class 12th

the lowest spin only magnetic moment for Ni⁺² because of minimum unpaired electron.

$Pb{\left(N{O}_3\right)}_2\underset{673K}{\overset{\Delta }{\to }}PbO+\underset{\left(A\right)}{N{O}_2}+O_2$

$\underset{\left(A\right)}{N{O}_2}\underset{}{\overset{Dimerise}{\to }}\underset{\left(B\right)}{N_2{O}_4}$

$E_{C{\mathcal{l}}_2/C{\mathcal{l}}^{-}}^0=+1.36V$

$E_{l_2/l^{-}}^0=+0.54V$

$E_{A{g}^{+}/Ag}^0=+0.80V$

$E_{N{a}^{+}/Na}^0=-2.71V$

$E_{L{i}^{+}/Li}^0=-3.05V$

$\therefore E_{C{\mathcal{l}}_2/C{\mathcal{l}}^{-}}^0>E_{A{g}^{+}/Ag}^0>E_{N{a}^{+}/Na}^0>E_{L{i}^{+}/Li}^0$

In electro-refining, impure metal (blister copper) is used as an anode while precious metal like Au, Pt gets deposited as anode mud.

Zymase naturally occurs in yeast.

Diastase is found in malt.

Urease is found in soyabean.

Pepsin is found in stomach.

Using snell's law –

sin I = $\mu sinr$

sin45° = $\mu sin30°$

$\mu$$=$$\frac{sin45}{sin30}$$=$$\frac{1}{\text{exception 25:}}$$*$$2$$=$√2

$B{i}_2{S}_3?{\underset{2S}{2Bi}}^{+3}+{\underset{3S}{3S}}^{-2}$

$Ksp={\left(2S\right)}^2{\left(3S\right)}^3=4*27*{\left(S\right)}^5$

= 108 (S)5

${\left(S\right)}^5=\frac{1.08*10^{-73}}{108}=10^{-75}$ $\therefore S=10^{-15}M$

$\Delta T_f=0.2°C$

$m=\frac{0.7*1000}{93*42}=\frac{700}{93*42}=0.179m$

$\Delta T_f=i{K}_{f}m$

$i=\frac{\Delta T_f}{K_f*m}=\frac{0.2}{1.86*0.179}=0.6$

$\frac{\alpha }{2}=1-0.6=0.4$

$\therefore \alpha =0.4*2=0.8$

% of = 80%

${?}_0=h{\upsilon }_0$

$=6.6*10^{-34}*1.3*10^{15}J$

$=8.58*10^{-19}J$

$l_g=nk$

$l_{g}G=\left(l-l_g\right)s$

$\Rightarrow nkG=\left(l-nk\right)s\Rightarrow l=\frac{nkG}{s}+nk=nk\frac{\left(G+s\right)}{s}$

$l=\frac{nk}{s}\left(G+s\right)$