Given the following cell reaction:
\(\mathrm{2Fe^{3+}(aq) \ + \ 2I^{-}(aq)\rightarrow 2Fe^{2+}(aq) \ + \ I_{2}(aq)}\)
The standard Gibbs energy ∆rG⊝ of the cell reaction is:
[Given: \(F = 96500\) \(C\) \(mol^{- 1}\)]
1. \(23 . 16\) \(kJ\) \(mol^{- 1}\)
2. \(- 46 . 32\) \(kJ\) \(mol^{- 1}\)
3. \(- 23 . 16\) \(kJ\) \(mol^{- 1}\)
4. \(46 . 32\) \(kJ\) \(mol^{- 1}\)
The manganate and permanganate ions are tetrahedral, due to:
| 1. | The π-bonding involves the overlap of d-orbitals of oxygen with d-orbitals of manganese. |
| 2. | The π-bonding involves the overlap of p-orbitals of oxygen with d-orbitals of manganese. |
| 3. | Absence of π-bonding. |
| 4. | The π-bonding involves the overlap of p-orbitals of oxygen with p-orbitals of manganese. |
1. CH3NH2 > (CH3)2NH > (CH3)3N
2. (CH3)2NH > CH3NH2 > (CH3)3N
3. (CH3)3N > CH3NH2 > (CH3)2NH
4. (CH3)2NH > (CH3)3N > CH3NH2
An alkene "A" on reaction with and gives propanone and ethanal in equimolar ratio. The addition of HCl to alkene "A" gives "B" as the major product. The structure of product "B" is:
| 1. |  |
2. |  |
| 3. |  |
4. |  |
For the second-period elements, the correct increasing order of first ionisation enthalpy is:
| 1. | Li < Be < B < C < O < N < F < Ne |
| 2. | Li < Be < B < C < N < O < F < Ne |
| 3. | Li < B < Be < C < O < N < F < Ne |
| 4. | Li < B < Be < C < N < O < F < Ne |
A gas at 350 K and 15 bar has a molar volume 20 percent smaller than that for an ideal gas under the same conditions. The correct option about the gas and its compressibility factor (Z) is:
| 1. | Z<1 and repulsive forces are dominant. |
| 2. | Z>1 and attractive forces are dominant. |
| 3. | Z>1 and repulsive forces are dominant. |
| 4. | Z<1 and attractive forces are dominant. |
For a cell involving one electron \(E_{cell}^{\ominus} = 0 . 59 V\) at 298 K. The equilibrium constant for the cell reaction is :
\(\mathrm{[Given~ that~ \frac {2.303 ~RT}{F} = 0.059 ~V~ at~ T = 298 K]}\)
| 1. | \(1 . 0 \times \left(10\right)^{30}\) | 2. | \(1 . 0 \times \left(10\right)^{2}\) |
| 3. | \(1 . 0 \times \left(10\right)^{5}\) | 4. | \(1 . 0 \times \left(10\right)^{10}\)
|
Which composition will make the basic buffer?
| 1. | 100 mL of 0.1 M HCl+100 mL of 0.1 M NaOH |
| 2. | 50 mL of 0.1 M NaOH+25 mL of 0.1 M CH3COOH |
| 3. | 100 mL of 0.1 M CH3COOH+100 mL of 0.1 M NaOH |
| 4. | 100 mL of 0.1 M HCl+200 mL of 0.1 M NH4OH |
The correct thermal stability order for \(\mathrm{{H}_2 {E}},\) \(\mathrm{{ E}= {O}, {S}, {Se}, {Te}} \text { and } \mathrm{Po}\) among the following is:
1. \(\mathrm{{H}_2 {Se}<{H}_2 {Te}<{H}_2 {Po}<{H}_2 {O}<{H}_2 S}\)
2. \(\mathrm{{H}_2 {~S}<{H}_2 {O}<{H}_2 {Se}<{H}_2 {Te}<{H}_2 {Po}}\)
3. \(\mathrm{{H}_2 {O}<{H}_2 {~S}<{H}_2 {Se}<{H}_2 {Te}<{H}_2 {PO}}\)
4. \(\mathrm{{H}_2 {Po}<{H}_2 {Te}<{H}_2 {Se}<{H}_2 {~S}<{H}_2 {O}}\)
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