- ✓$\Delta H =\Delta U - P \Delta V$
- B$\Delta U = q + W$
- C$\Delta S _{ syz }+\Delta S _{ suxr } \geq 0$
- D$\Delta G =\Delta H - T \Delta S$
$\Delta 14=\Delta U +\Delta( Pr )$ at constant pressure
$\Delta H =\Delta U + P \Delta V$
Generate a complete, print-ready paper with questions like this in minutes — across 16+ boards, with answer keys.
The rate constants of the above reaction at $200 \,K$ and $300 \,K$ are $0.03 \,min ^{-1}$ and $0.05 \,min ^{-1}$ respectively. The activation energy for the reaction is $....J$ (Nearest integer)
(Given : In $10=2.3$
$R =8.3\,J\,K ^{-1}\, mol ^{-1}$
$\log 5=0.70$
$\log 3=0.48$
$\log 2=0.30$
(Given Atomic No. of $\mathrm{Ho}=67$ )
$Al_{(S)}+3Ag^+_{(aq)}\,(0.10\, M) \to Al^{+3}_{(aq)}\, (0.30\, M)+3Ag_{(S)}$,
the measured voltage $(E_{cell})$ is $1.50\, volt$. Calculate $E_{cell}^o$ ........... $\mathrm{volt}$
Given : $\frac{{2.303\,RT}}{F} = 0.06\,;\,\log \,3 = 0.48$

$(A)$ $\Delta G$ is positive $(B)$ $\Delta S _{\text {system }}$ is positive
$(C)$ $\Delta S _{\text {surroundings }}=0$ $(D)$ $\Delta H =0$