MCQ
Lewis base is
- A$C{O_2}$
- B$S{O_3}$
- C$S{O_2}$
- ✓$ROH$
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$(I)$ $CO_2$ $(II)$ $Br_2$ $(III)$ $SnCl_2$ $(IV)$ $HF$ $(V)$ $NMe_3$
The following data are observed
| $[X_2]$ | $[Y_2]$ | Rate of appearance of $XY$ ($M/sec$) |
| $0.1$ | $0.1$ | $5 × 10^{-6}$ |
| $0.2$ | $0.1$ | $10^{-5}$ |
| $0.2$ | $0.2$ | $4 × 10^{-5}$ |
Rate constant of reaction will (in $M^{1-n}\,sec^{-1}$) where $'n'$ is order of reaction
Statement- $I$: Along the period, the chemical reactivity of the element gradually increases from group $1$ to group $18$.
Statement - $II$: The nature of oxides formed by group $1$ element is basic while that of group $17$ elements is acidic.In the the light above statements, choose the most appropriate from the questions given below:
$(i)$ $H_{(aq)}^+ + OH^-= H_2O_{(l)} ,$ $\Delta H = -X_1\,kJ \,mol^{-1}$
$(ii)$ $H_{2(g)} + \frac{1}{2}O_{2(g)} = H_2O_{(l)},$ $\Delta H = -X_2\,kJ \,mol^{-1}$
$(iii)$ $CO_{2(g)} + H_{2(g)} = CO_{(g)} + H_2O_{(l)},$ $\Delta H = -X_3\, kJ\, mol^{-1}$
$(iv)$ $ C_2H_{2(g)}+ \frac{5}{2} O_{2(g)} = 2CO_{2(g)} + H_2O_{(l)},$ $\Delta H = -X_4\,kJ \,mol^{-1}$
Enthalpy of formation of $H_2O_{(l)}$ is