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| Acid | $HF$ | $HCL$ | $HBr$ | $HI$ |
| $K_a$ | $7.2 \times 10^{-4}$ | $1 \times 10^6$ | $1 \times 10^9$ | $3 \times 10^{11}$ |
Which of these Bronsted acids would have the weakest conjugate base ?
$O(g) + e^- = O^-(g)$ $\Delta {H_{eg}} = - 142\,kJ\,mo{l^{ - 1}}$
$O^-(g) + e^- = O^{2-}(g)$ $\Delta {H_{eg}} = +844\,kJ\,mo{l^{ - 1}}$
This is because
$2 A ( g ) \rightleftharpoons A _{2}( g )$
at $400\, K$ has $\Delta G ^{\circ}=+25.2\, kJ mol ^{-1}$.
The equilibrium constant $K _{ C }$ for this reaction is $...... \times 10^{-2}$. (Round off to the Nearest integ $\left[\right.$ Use $: R=8.3\, J mol ^{-1} K ^{-1}, \ln 10=2.3$
$\left.\log _{10} 2=0.30,1\, atm =1\, bar \right]$
$[$ antilog $(-0.3)=0.501]$
${N_2}{H_4}(l)\,+\,2{H_2}{O_2}(l)\,\, \to \,{N_2}(g)\,\, + \,4{H_2}O(l);\,\,{\Delta _r}H_1^o\, = \, - 818\,\,kJ/mol$
${N_2}{H_4}(l)\,\, + {O_2}(g)\,\, \to \,{N_2}(g)\,\, + \,2{H_2}O(l);\,\,{\Delta _r}H_2^o\, = \, - 622\,\,kJ/mol$
${H_2}(g)\,\, + 1/2{O_2}(g)\,\, \to \,{H_2}O(l);\,\,{\Delta _r}H_3^o\, = \, - 285\,\,kJ/mol$
......$kJ/mol$