Question
In an equilibrium reaction for which $\Delta {G^o} = 0$, the equilibrium constant $K = $
$\Delta {G^o} = - 2.303\,\,RT\,\,\log \,{K_p}$
$\log \,{K_p} = 0$
${K_p} = 1$.
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$\mathrm{HF}, \mathrm{H}_2 \mathrm{O}, \mathrm{SO}_2, \mathrm{H}_2, \mathrm{CO}_2, \mathrm{CH}_4, \mathrm{NH}_3, \mathrm{HCl}, \mathrm{CHCl}_3, \mathrm{BF}_3$
$H _{2} F _{2( g )} \rightarrow H _{2( g )}+ F _{2( g )}$
$\Delta U =-59.6\,kJ\,mol ^{-1} \text { at } 27^{\circ}\,C$.
The enthalpy change for the above reaction is (-) $kJ mol ^{-1}$ [nearest integer] Given : $R =8.314\,JK ^{-1}\,mol ^{-1}$
$N _2 O _3, N _2 O _5, P _4 O _6, P _4 { O }_7, H _4 P _2 O _5, H _5 P _3 O _{10}, H _2 S _2 O _3, H _2 S _2 O _5$