- A$[Fe(CN)_6]^{3-}$
- ✓$Fe_2(SO_4)_3$
- C$[Fe(CN)_6]^{4-}$
- D$(NH_4)_2SO_4. FeSO_4.6H_2O$
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$C{H_2} = CH{(C{H_2})_8}COOH + HBr\xrightarrow{{peroxide}}....$
${C_6}{H_5}N{O_2}\xrightarrow{{Sn / HCl}}X\xrightarrow{{{C_6}{H_5}COCl}}Y + HCl$
What is $Y$ ?
$[A]$ With increase in temperature, the value of $K$ for exothermic reaction decreases because entropy change of the system is positive
$[B]$ With increase in temperature, the value of $K$ for endothermic reaction increases because unfavourable change in entropy of the surroundings decreases
$[C]$ With increase in temperature, the value of $K$ for endothermic reaction increases because the entropy change of the system is negative
$[D]$ With increase in temperature, the value of $K$ for exothermic reaction decreases because favourable change in entropy of the surrounding decreases
