Question:
In acidic medium, dichromate ion oxidises ferrous ion to ferric ion. If the gram molecular weight of potassium dichromate is 294 g, its gram equivalent weight is ...... g.
In acidic medium, dichromate ion oxidises ferrous ion to ferric ion. If the gram molecular weight of potassium dichromate is 294 g, its gram equivalent weight is ...... g.
Updated On: May 21, 2024
- 294
- 147
- 49
- 24.5
Hide Solution
Verified By Collegedunia
The Correct Option is C
Solution and Explanation
The reaction of dichromate ion with ferrous ion in acidic medium takes place as: $ 6F{{e}^{2+}}+C{{r}_{2}}O_{7}^{2-}+14{{H}^{+}}\xrightarrow{{}} $ $ 6{{F}^{3+}}+2C{{r}^{3+}}+7{{H}_{2}}O $ Total change in oxidation state of iron is $ \overset{+12}{\mathop{6F{{e}^{2+}}}}\,\xrightarrow{{}}\overset{+18}{\mathop{6F{{e}^{3+}}}}\, $ Total change = + 6 So, gram equivalent weight of $ {{K}_{2}}C{{r}_{2}}{{O}_{7}} $ $ \text{=}\,\,\frac{\text{294}}{\text{Total}\,\text{change}\,\text{in}\,\text{O}\text{.S}} $ $ =\frac{294}{6}=49\,g $
Was this answer helpful?
1
0
Top Questions on d block elements
- The electronic configuration of Cu(II) is 3d9 whereas that of Cu(I) is 3d10. Which of the following is correct ?
- JEE Main - 2024
- Chemistry
- d block elements
- The correct statement(s) about the ligand substitution/exchange reaction is/are
- IIT JAM CY - 2024
- Inorganic Chemistry
- d block elements
- Among [Ti(H2O)6]3+,[NiCl4]2−,[CrO4]2−,and [Mn(H2O)6]2+, the complex that exhibits the largest molar absorptivity in the visible region of the electronic absorption spectrum is
- IIT JAM CY - 2024
- Inorganic Chemistry
- d block elements
- [Co(NH3)5(SO4)]Br and [Co(NH3)5Br]SO4 are examples of
- IIT JAM CY - 2024
- Inorganic Chemistry
- d block elements
- For the reaction shown below
![1/2 Mn2 (CO)10+Na Na[Mn(CO)5 ] CH3Cl-NaCl [CH3Mn(CO)5](https://images.collegedunia.com/public/qa/images/content/2024_07_31/image_a08f12a11722411541392.png)
the oxidation states of Mn in P and Q, respectively, are- IIT JAM CY - 2024
- Inorganic Chemistry
- d block elements
View More Questions
Questions Asked in EAMCET exam
- If $\quad \tan \theta \cdot \tan \left(120^{\circ}-\theta\right) \tan \left(120^{\circ}+\theta\right)=\frac{1}{\sqrt{3}}$, then $\theta$ is equal to
- EAMCET - 2015
- Trigonometric Equations
- If $f: R \rightarrow R, g: R \rightarrow R$ are defined by $f(x)=5\, x-3, g(x)=x^{2}+3$, then $g o f^{-1}(3)$ is equal to
- EAMCET - 2015
- Differentiability
- The common roots of the equations $z^{3}+2 z^{2}+2 z+1=0, z^{2014}+z^{2015}+1=0$ are
- EAMCET - 2015
- Quadratic Equations
- The value of the sum $1 \cdot 2 \cdot 3+2 \cdot 3 \cdot 4+3 \cdot 4 \cdot 5+\ldots$ upto $n$ terms is equal to
- EAMCET - 2015
- Sum of First n Terms of an AP
- The system $2\,x+3 y+z=5,3\,x+y+5\,z=7$ and $x+4\,y-2\,z=3$ has
- EAMCET - 2015
- Transpose of a Matrix
View More Questions
Concepts Used:
d block elements
The elements, in the columns of the periodic table in which d subshells are being occupied are known as d block elements.
These are the elements that have the capability of forming stable cations with incompletely filled d orbitals. Elements like mercury and Zinc are not considered transition metals because they have electronic configurations: (n-1)d10 ns2. These elements have filled d-orbitals in their ground state and, therefore, even in some of their oxidation states.
General Properties Of d-Block Elements
- Multiple oxidation states- The oxidation states of d block elements show very few energy gaps; therefore, they exhibit many oxidation states. Also, the energy difference between s and d orbital is very less. Therefore both the electrons are involved in ionic and covalent bond formation, which ultimately leads to multiple oxidation states.
- Formation of complex compounds- Ligands show a binding behaviour and can form so many stable complexes with the help of transition metals. This property is mainly due to:
- Availability of vacant d orbitals.
- Comparatively small sizes of metals.
- Hardness- Transition elements are tough and have high densities because of the presence of unpaired electrons.
- Melting and boiling points- Melting and boiling points of transition are very high. This is because of the presence of unpaired electrons and partially filled d orbitals. Because of these two things, they form strong bonds and therefore have high melting and boiling points.
- Atomic radii- The atomic and ionic radius of the transition elements decreases as we move from Group 3 to group 6. However, it remains the same between group 7 and group 10, and from group 11 to group 12 increases.
- Ionization enthalpy- The ionization enthalpies of the transition elements are generally on the greater side as compared to the S block elements