A peptide synthesized by the reactions of one molecule each of Glycine

Question: A peptide synthesized by the reactions of one molecule each of Glycine, Leucine, Aspartic acid and Histidine will have peptide linkages. Solution: Total (3) peptide linkages are present 3 peptide linkage Ans. (3)...

If the conductivity of mercury at

Question: If the conductivity of mercury at $0^{\circ} \mathrm{C}$ is $1.07 \times 10^{6}$ $\mathrm{S} \mathrm{m}^{-1}$ and the resistance of a cell containing mercury is $0.243 \Omega$, then the cell constant of the cell is $\mathrm{x} \times 10^{4} \mathrm{~m}^{-1}$. The value of $\mathrm{x}$ is .(Nearest integer) Solution: $\mathrm{k}=1.07 \times 10^{6} \mathrm{Sm}^{-1}, \quad \mathrm{R}=0.243 \Omega$ $\mathrm{G}=\frac{1}{\mathrm{R}}=\frac{1}{0.243} \Omega^{-1}$ $\mathrm{k}=\mathrm{G} \times ...

The spin-only magnetic moment value of

Question: The spin-only magnetic moment value of $\mathrm{B}_{2}^{+}$ species is $\times 10^{-2} \mathrm{BM}$. (Nearest integer) [Given : $\sqrt{3}=1.73$ ] Solution: $\mathrm{B}_{2}^{+} \Rightarrow \sigma_{1 \mathrm{~s}}^{2} \sigma_{1 \mathrm{~s}}^{* 2} \sigma_{2 \mathrm{~s}}^{2} \sigma_{2 \mathrm{~s}}^{* 2} \pi_{2 p y}^{1} \simeq \pi_{2 p z}^{0}$ $\Rightarrow 9 \mathrm{e}^{-}$ $\mu=\sqrt{1(1+2)}=\sqrt{3} \mathrm{BM}$ $=1.73 \mathrm{BM}$ $=1.73 \times 10^{-2} \mathrm{BM}$...

A 50 watt bulb emits monochromatic red light of wavelength of

Question: A 50 watt bulb emits monochromatic red light of wavelength of $795 \mathrm{~nm}$. The number of photons emitted per second by the bulb is $\mathrm{x} \times 10^{20}$. The value of $x$ is $\left[\right.$ Given : $\mathrm{h}=6.63 \times 10^{-34} \mathrm{JS}$ and $\left.\mathrm{c}=3.0 \times 10^{8} \mathrm{~ms}^{-1}\right]$ Solution: Total energy per sec. $=50 \mathrm{~J}$ $50=\frac{\mathrm{n} \times 6.63 \times 10^{-34} \times 3 \times 10^{8}}{795 \times 10^{-9}}$ $\mathrm{n}=1998.49 \ti...

Solve this following

Question: If $80 \mathrm{~g}$ of copper sulphate $\mathrm{CuSO}_{4} \cdot 5 \mathrm{H}_{2} \mathrm{O}$ is dissolved in deionised water to make $5 \mathrm{~L}$ of solution. The concentration of the copper sulphate solution is $\mathrm{x} \times 10^{-3} \mathrm{~mol} \mathrm{~L}^{-1}$. The value of $\mathrm{x}$ is [Atomic masses $\mathrm{Cu}: 63.54 \mathrm{u}, \mathrm{S}: 32 \mathrm{u}, \mathrm{O}: 16 \mathrm{u}, \mathrm{H}: 1 \mathrm{u}$ ] Solution: Moles of $\mathrm{CuSO}_{4} \cdot 5 \mathrm{H}_...

The number of atoms in

Question: The number of atoms in $8 \mathrm{~g}$ of sodium is $\mathrm{x} \times 10^{23}$. The value of $x$ is .(Nearest integer) [Given : $\mathrm{N}_{\mathrm{A}}=6.02 \times 10^{23} \mathrm{~mol}^{-1}$ Atomic mass of $\mathrm{Na}=23.0 \mathrm{u}]$ Solution: No. of atoms $=\frac{8}{23} \times 6.02 \times 10^{23}=2.09 \times 10^{23}$ $\simeq 2 \times 10^{23}$ $=x \times 10^{23}$ $x=2$...

The sum of oxidation states of two silver ions in

Question: The sum of oxidation states of two silver ions in $\left[\mathrm{Ag}\left(\mathrm{NH}_{3}\right)_{2}\right]\left[\mathrm{Ag}(\mathrm{CN})_{2}\right]$ complex is Solution:...

Solve this following

Question: For the reaction $2 \mathrm{NO}_{2}(\mathrm{~g}) \rightleftharpoons \mathrm{N}_{2} \mathrm{O}_{4}(\mathrm{~g})$, when $\Delta \mathrm{S}=-176.0 \mathrm{JK}^{-1}$ and $\Delta \mathrm{H}=-57.8 \mathrm{~kJ} \mathrm{~mol}^{-1}$, the magnitude of $\Delta \mathrm{G}$ at $298 \mathrm{~K}$ for the reaction is $\mathrm{kJ} \mathrm{mol}^{-1}$. (Nearest integer) Solution: $\Delta \mathrm{G}=\Delta \mathrm{H}-\mathrm{T} \Delta \mathrm{S}$ $\Delta \mathrm{G}=57.8-\frac{298(-176)}{1000}$ $\Delta \ma...

Solve this following

Question: The molar solubility of $\mathrm{Zn}(\mathrm{OH})_{2}$ in $0.1 \mathrm{M} \mathrm{NaOH}$ solution is $\mathrm{x} \times 10^{-18} \mathrm{M}$. The value of $\mathrm{x}$ is (Given : The solubility product of $\mathrm{Zn}(\mathrm{OH})_{2}$ is $2 \times 10^{-20}$ ) Solution: $\mathrm{Zn}(\mathrm{OH})_{2}(\mathrm{~s}) \rightleftharpoons \mathrm{Zn}^{+2}(\mathrm{aq})+2 \mathrm{OH}$ (aq) $(0.1+2 \mathrm{~s})=0.1$ $\mathrm{K}_{\mathrm{sp}}=\mathrm{S}(0.1)^{2}$ $2 \times 10^{-20}=\mathrm{s} \ti...

Question: The molar solubility of $\mathrm{Zn}(\mathrm{OH})_{2}$ in $0.1 \mathrm{M} \mathrm{NaOH}$ solution is $\mathrm{x} \times 10^{-18} \mathrm{M}$. The value of $\mathrm{x}$ is (Given : The solubility product of $\mathrm{Zn}(\mathrm{OH})_{2}$ is $2 \times 10^{-20}$ ) Solution: $\mathrm{Zn}(\mathrm{OH})_{2}(\mathrm{~s}) \rightleftharpoons \mathrm{Zn}^{+2}(\mathrm{aq})+2 \mathrm{OH}$ (aq) $(0.1+2 \mathrm{~s})=0.1$ $\mathrm{K}_{\mathrm{sp}}=\mathrm{S}(0.1)^{2}$ $2 \times 10^{-20}=\mathrm{s} \ti...

An empty LPG cylinder weighs

Question: An empty LPG cylinder weighs $14.8 \mathrm{~kg}$. When full, it weighs $29.0 \mathrm{~kg}$ and shows a pressure of $3.47$ $\mathrm{atm}$. In the course of use at ambient temperature, the mass of the cylinder is reduced to $23.0 \mathrm{~kg}$. The final pressure inside of the cylinder is atm. (Nearest integer) (Assume LPG of be an ideal gas) Solution: Initial mass of gas $=29-14.8=14.2 \mathrm{Kg}$ mass of gas used $=29-23=6 \mathrm{Kg}$ gas left $=14.2-6=8.2 \mathrm{Kg}$ (1) $3.47 \tim...

Identify the element for which electronic configuration in

Question: Identify the element for which electronic configuration in $+3$ oxidation state is $[\mathrm{Ar}] 3 \mathrm{~d}^{5}:$$\mathrm{Ru}$$\mathrm{Mn}$$\mathrm{Co}$$\mathrm{Fe}$Correct Option: , 4 Solution: $\mathrm{Fe}^{3+}[\mathrm{Ar}] 3 \mathrm{~d}^{5}$...

Number of paramagnetic oxides among the following given oxides is

Question: Number of paramagnetic oxides among the following given oxides is $\mathrm{Li}_{2} \mathrm{O}, \mathrm{CaO}, \mathrm{Na}_{2} \mathrm{O}_{2}, \mathrm{KO}_{2}, \mathrm{MgO}$ and $\mathrm{K}_{2} \mathrm{O}$1230Correct Option: 1 Solution: $\mathrm{Li}, \mathrm{O} \Rightarrow 2 \mathrm{Li}^{+} \quad \mathrm{O}^{2-}$ $\mathrm{MgO} \Rightarrow \mathrm{Mg}^{2+} \mathrm{O}^{2-}$ $\mathrm{CaO} \Rightarrow \mathrm{Ca}^{2+} \quad \mathrm{O}^{2-}$ $\mathrm{K}_{2} \mathrm{O} \Rightarrow 2 \mathrm{~K...

solve this

Question: $\left[\mathrm{Ti}\left(\mathrm{H}_{2} \mathrm{O}\right)_{6}\right]^{3+}$ absorbs light of wavelength 498 $\mathrm{nm}$ during a $\mathrm{d}-\mathrm{d}$ transition. The octahedral splitting energy for the above complex is__________ $\times 10^{-19} \mathrm{~J}$. (Round off to the Nearest Integer). $\mathrm{h}$ $=6.626 \times 10^{-34} \mathrm{~J} \mathrm{~s} ; \mathrm{c}=3 \times 10^{8} \mathrm{~ms}^{-1}$. Solution: $\lambda_{\text {absorbed }}=498 \mathrm{~nm}$ (given) The octahedral s...

The oxide without nitrogen-nitrogen bond is :

Question: The oxide without nitrogen-nitrogen bond is : $\mathrm{N}_{2} \mathrm{O}$$\mathrm{N}_{2} \mathrm{O}_{4}$$\mathrm{N}_{2} \mathrm{O}_{3}$$\mathrm{N}_{2} \mathrm{O}_{5}$Correct Option: , 4 Solution:...

solve this

Question: At $25^{\circ} \mathrm{C}, 50 \mathrm{~g}$ of iron reacts with $\mathrm{HCl}$ to form $\mathrm{FeCl}_{2}$. The evolved hydrogen gas expands against a constant pressure of 1 bar. The work done by the gas during this expansion is_____________J (Round off to the Nearest Integer) [Given : $\mathrm{R}=8.314 \mathrm{~J} \mathrm{~mol}^{-1} \mathrm{~K}^{-1}$. Assume, hydrogen is an ideal gas] [Atomic mass off $\mathrm{Fe}$ is $55.85 \mathrm{u}$ ] Solution: $\mathrm{T}=298 \mathrm{~K}, \mathrm{...

A chloro compound "A".

Question: A chloro compound "A". (i) forms aldehydes on ozonolysis followed by the hydrolysis. (ii) when vaporized completely $1.53 \mathrm{~g}$ of A, gives $448 \mathrm{~mL}$ of vapour at STP. The number of carbon atoms in a molecule of compound $\mathbf{A}$ is Solution: $448 \mathrm{ml}$ of $\mathrm{A} \Rightarrow 1.53 \mathrm{gm} \mathrm{A}$ $22400 \mathrm{ml}$ of $\mathrm{A} \Rightarrow \frac{1.53}{445} \times 22400 \mathrm{gm} \mathrm{A}=7650$ $\ \mathrm{~mm}$ is $36+5+35.5=76.5$ 26 August ...

The reaction rate for the reaction

Question: The reaction rate for the reaction $\left[\mathrm{PtCl}_{4}\right]^{2-}+\mathrm{H}_{2} \mathrm{O} \rightleftharpoons\left[\mathrm{Pt}\left(\mathrm{H}_{2} \mathrm{O}\right) \mathrm{Cl}_{3}\right]^{-}+\mathrm{Cl}^{-}$ was measured as a function of concentrations of different species. It was observed that $\frac{-\mathrm{d}\left[\left[\mathrm{PtCl}_{4}\right]^{2-}\right]}{\mathrm{dt}}=4.8 \times 10^{-5}\left[\left[\mathrm{PtCl}_{4}\right]^{2-}\right]-2.4 \times$ $10^{-3}\left[\left[\mathr...

The potassium ferrocyanide solution gives a Prussian blue colour, when added to :

Question: The potassium ferrocyanide solution gives a Prussian blue colour, when added to :$\mathrm{CoCl}_{3}$$\mathrm{FeCl}_{2}$$\mathrm{CoCl}_{2}$$\mathrm{FeCl}_{3}$Correct Option: , 4 Solution: $\mathrm{FeCl}_{3}+\mathrm{K}_{4}\left[\mathrm{Fe}(\mathrm{CN})_{6}\right] \rightarrow \mathrm{Fe}_{4}\left[\mathrm{Fe}(\mathrm{CN})_{6}\right]_{3}$ Prussian blue...

83g of ethylene glycol dissolved

Question: $83 \mathrm{~g}$ of ethylene glycol dissolved in $625 \mathrm{~g}$ of water. The freezing point of the solution is $\mathrm{K} .$ (Nearest integer) [Use : Molal Freezing point depression constant of water $=1.86 \mathrm{~K} \mathrm{~kg} \mathrm{~mol}^{-1}$ ] Freezing Point of water $=273 \mathrm{~K}$ Atomic masses : $\mathrm{C}: 12.0 \mathrm{u}, \mathrm{O}: 16.0 \mathrm{u}, \mathrm{H}: 1.0 \mathrm{u}]$ Solution: $\mathrm{k}_{\mathrm{f}}=1.86 \mathrm{k} . \mathrm{kg} / \mathrm{mol}$ $\m...

When 35 mL of 0.15 M lead nitrate solution

Question: When $35 \mathrm{~mL}$ of $0.15 \mathrm{M}$ lead nitrate solution is mixed with $20 \mathrm{~mL}$ of $0.12 \mathrm{M}$ chromic sulphate solution,_____________ $\times 10^{-5}$ moles of lead sulphate precipitate out. (Round off to the Nearest Integer). Solution: $3 \mathrm{~Pb}\left(\mathrm{NO}_{3}\right)_{2}+\mathrm{Cr}_{2}\left(\mathrm{SO}_{4}\right)_{3} \rightarrow 3 \mathrm{PbSO}_{4}+2 \mathrm{Cr}\left(\mathrm{NO}_{3}\right)_{3}$ $\begin{array}{ll}35 \mathrm{ml} 20 \mathrm{ml} \\ 0....

The overall stability constant

Question: The overall stability constant of the complex ion $\left[\mathrm{Cu}\left(\mathrm{NH}_{3}\right)_{4}\right]^{2+}$ is $2.1 \times 10^{13}$. The overall dissociations constant is $\mathrm{y} \times 10^{-14}$. Then $\mathrm{y}$ is .(Nearest integer) Solution: Given $\mathrm{k}_{\mathrm{f}}=2.1 \times 10^{13}$ $\mathrm{K}_{\mathrm{d}}=\frac{1}{\mathrm{k}_{\mathrm{f}}}=4.7 \times 10^{-14}$ $\therefore y=4.7 \approx 5$...

Which one of the following gives the most stable Diazonium salt?

Question: Which one of the following gives the most stable Diazonium salt? $\mathrm{CH}_{3}-\mathrm{CH}_{2}-\mathrm{CH}_{2}-\mathrm{NH}_{2}$Correct Option: , 2 Solution:...

Solve the following equations

Question: $100 \mathrm{~mL}$ of $\mathrm{Na}_{3} \mathrm{PO}_{4}$ solution contains $3.45 \mathrm{~g}$ of sodium. The molarity of the solution is $\times 10^{-2}$ $\mathrm{mol} \mathrm{L}^{-1}$. (Nearest integer) [Atomic Masses - $\mathrm{Na}: 23.0 \mathrm{u}, \mathrm{O}: 16.0 \mathrm{u}, \mathrm{P}: 31.0 \mathrm{u}$ ] Solution: therefore molarity of $\mathrm{Na}_{3} \mathrm{PO}_{4}$ Solution $=$ $\frac{\mathrm{n}_{\mathrm{Na}_{3} \mathrm{PO}_{4}}}{\text { volume of solution in } \mathrm{L}}$ $=...

For the galvanic cell,

Question: For the galvanic cell, $\mathrm{Zn}(\mathrm{s})+\mathrm{Cu}^{2+}(0.02 \mathrm{M}) \rightarrow \mathrm{Zn}^{2+}(0.04 \mathrm{M})+\mathrm{Cu}(\mathrm{s})$ $\mathrm{E}_{\mathrm{cell}}=\longrightarrow \times 10^{-2} \mathrm{~V} .$ (Nearest integer) $\left[\right.$ Use : $\mathrm{E}_{\mathrm{Cu} / \mathrm{Cu}^{2+}}^{0}=-0.34 \mathrm{~V}, \mathrm{E}_{\mathrm{Zn} / \mathrm{Zn}^{2+}}^{0}=+0.76 \mathrm{~V},$, $\left.\frac{2.303 \mathrm{RT}}{\mathrm{F}}=0.059 \mathrm{~V}\right]$ Solution: Galvan...