MCQ
Order of decreasing basic strengths of halides is
- A$F^- > Cl^- > I^- > Br^-$
- ✓$F^- > Cl^- > Br^- > I^-$
- C$I^- > Br^- > Cl^- > F^-$
- D$I^- > Cl^- > Br^- > F^-$
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$\frac{d[NH_3]}{dt} = 2 \times 10^{-4} \, mol \,L^{-1} \, s^{-1}$ , the value of $\frac{-d[H_2]}{dt}$ would be .................. $mol \,L^{-1} \, s^{-1}$
$H_2 + F_2 \longrightarrow 2HF$
given that
Bond energy of $H-H$ bond $= 434\, kJ/mol$
Bond energy of $F-F$ bond $= 158\, kJ/mol$
Bond energy of $H-F$ bond $= 565\, kJ/mol$
.....$ kJ$