Recent questions tagged unit2

At room temperature $25^{\large\circ}C$,the vapour pressure of pure methyl alcohol is 90 torr.Mol fraction of $CH_3OH$ in a solution in which vapour pressure of $CH_3OH$ is 20 torr at $25^{\large\circ}$ is ?

asked Feb 14, 2014 by sreemathi.v

1 answer

Most likely the following mixtures to be an ideal solution is

asked Feb 14, 2014 by sreemathi.v

1 answer

At room temperature $25^{\large\circ}C$,the expression for total pressure of mixture of methanol and ethanol solution is given by P(in torr)$=135+120X$ where $X$ is mol fraction of methanol,Hence

asked Feb 14, 2014 by sreemathi.v

1 answer

When mercuric iodide is added to the aqueous solution of potassium iodide,the

asked Feb 14, 2014 by sreemathi.v

3 answers

Mixture of volatile components A and B has total vapour pressure (in torr) P=$250-115X_A$ where $X_A$ is mol fraction of 'A' in mixture.Hence $P_A^0$ and $P_B^0$ respectively are (in torr)

asked Feb 14, 2014 by sreemathi.v

1 answer

Which of the following azeotropic solutions has the boiling point less than the boiling point of the constituents

asked Feb 14, 2014 by sreemathi.v

1 answer

An azeotropic solution of two liquids has a boiling point lower than either of them when it

asked Feb 14, 2014 by sreemathi.v

2 answers

Which is true about enthalpy of solution containing benzene and toluene?

asked Feb 14, 2014 by sreemathi.v

1 answer

The degree of dissociation $'\alpha'$ of a weak electrolyte is (N is number of ions given by 1 mol of the electrolyte)

asked Feb 14, 2014 by sreemathi.v

1 answer

Which of the following has maximum freezing point for 1 molal solution, assuming equal ionisation in each case?

asked Feb 14, 2014 by sreemathi.v

1 answer

One mole each of the following solutes are taken in 1000g of water

asked Feb 14, 2014 by sreemathi.v

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Lowering of vapour pressure due to a solute in 1 molal aqueous solutions at $100^{\large\circ}C$ is

asked Feb 14, 2014 by sreemathi.v

1 answer

Match the column-I with column-II ,which are true for 20% w/w aqueous KI solution (density of KI solution is 1.20g/ml & M.wt of KI is 166 g/mol)

asked Feb 14, 2014 by sreemathi.v

1 answer

Match the column-I and column-II

asked Feb 14, 2014 by sreemathi.v

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Which is true about ideal solutions?

asked Feb 14, 2014 by sreemathi.v

1 answer

Total vapour pressure of mixture of 1 mole $X(P_x^0=150torr)$ and 2 mol Y$(P_y^0=240torr)$ is 210mm.In this case

asked Feb 14, 2014 by sreemathi.v

1 answer

A binary liquid solution is prepared by mixing n-heptane and ethanol.Which one of the following statements is correct regarding the behaviour of the solution?

asked Feb 13, 2014 by sreemathi.v

1 answer

Which of the following aqueous solutions posses zero as Van't Hoff coefficient?

asked Feb 13, 2014 by sreemathi.v

1 answer

The osmotic pressures of equimolar solutions of glucose, potassium chloride and Barium chloride will be in the order

asked Feb 13, 2014 by sreemathi.v

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Two aqueous solution X and Y are separated by a semipermeable membrane.If the vapour pressure of solution X is greater than the vapour pressure of solution Y,then the solvent water

asked Feb 12, 2014 by sreemathi.v

1 answer

Molarity of NaOH solution containing 5g of NaOH in 450ml of solution?

asked Feb 12, 2014 by sreemathi.v

1 answer

The hydrogen-like species $Li^{2+}$ is in a spherically symmetric state $S_1$ with one radial node. Upon absorbing light the ion undergoes transition to a state $S_2$ has one radial node and its energy is equal to the ground state energy of hydrogen atom. The orbital angular momentum quantum number of the state $S_2$ is

asked Feb 10, 2014 by sharmaaparna1

1 answer

The hydrogen-like species $Li^{2+}$ is in a spherically symmetric state $S_1$ with one radial node. Upon absorbing light the ion undergoes transition to a state $S_2$ has one radial node and its energy is equal to the ground state energy of hydrogen atom. Energy of the state $S_1$ in units of the hydrogen atom ground state energy is

asked Feb 10, 2014 by sharmaaparna1

1 answer

The hydrogen-like species $Li^{2+}$ is in a spherically symmetric state $S_1$ with one radial node. Upon absorbing light the ion undergoes transition to a state $S_2$ has one radial node and its energy is equal to the ground state energy of hydrogen atom. The state $S_1$ is

asked Feb 10, 2014 by sharmaaparna1

1 answer

De-Broglie proposed dual nature for electron by putting his famous equation $\lambda = \large\frac{h}{mu}$. Later on Heisenburg proposed uncertainity principle as $\bigtriangleup p .\bigtriangleup x \geq \large\frac{h}{2}(h = \large\frac{h}{2\pi})$ . On the contrary particle nature of electron was established on the basis of photoelectric effect. When a photon strikes the metal surface , it gives up its energy to the electron. Part of this energy (say w) is used by the electron to escape from the metal and the remaining imparts the kinetic energy $\large\frac{1}{2}mu^2$ to the photoelectron. The potential applied on the surface to reduce the velocity of photoelectron to zero is known as stopping potential. The wavelength of a golf ball weighing 200g and moving at a speed of 5meter/hr is of the order:

asked Feb 10, 2014 by sharmaaparna1

1 answer

De-Broglie proposed dual nature for electron by putting his famous equation $\lambda = \large\frac{h}{mu}$. Later on Heisenburg proposed uncertainity principle as $\bigtriangleup p .\bigtriangleup x \geq \large\frac{h}{2}(h = \large\frac{h}{2\pi})$ . On the contrary particle nature of electron was established on the basis of photoelectric effect. When a photon strikes the metal surface , it gives up its energy to the electron. Part of this energy (say w) is used by the electron to escape from the metal and the remaining imparts the kinetic energy $\large\frac{1}{2}mu^2$ to the photoelectron. The potential applied on the surface to reduce the velocity of photoelectron to zero is known as stopping potential. If uncertainities in position and momentum of an electron are same , then uncertainity in its velocity can be given by

asked Feb 10, 2014 by sharmaaparna1

1 answer

De-Broglie proposed dual nature for electron by putting his famous equation $\lambda = \large\frac{h}{mu}$. Later on Heisenburg proposed uncertainity principle as $\bigtriangleup p .\bigtriangleup x \geq \large\frac{h}{2}(h = \large\frac{h}{2\pi})$ . On the contrary particle nature of electron was established on the basis of photoelectric effect. When a photon strikes the metal surface , it gives up its energy to the electron. Part of this energy (say w) is used by the electron to escape from the metal and the remaining imparts the kinetic energy $\large\frac{1}{2}mu^2$ to the photoelectron. The potential applied on the surface to reduce the velocity of photoelectron to zero is known as stopping potential. The binding energy of electron in a metal is 250 KJ/mol. The threshold frequency of metal is

asked Feb 10, 2014 by sharmaaparna1

1 answer

De-Broglie proposed dual nature for electron by putting his famous equation $\lambda = \large\frac{h}{mu}$. Later on Heisenburg proposed uncertainity principle as $\bigtriangleup p .\bigtriangleup x \geq \large\frac{h}{2}(h = \large\frac{h}{2\pi})$ . On the contrary particle nature of electron was established on the basis of photoelectric effect. When a photon strikes the metal surface , it gives up its energy to the electron. Part of this energy (say w) is used by the electron to escape from the metal and the remaining imparts the kinetic energy $\large\frac{1}{2}mu^2$ to the photoelectron. The potential applied on the surface to reduce the velocity of photoelectron to zero is known as stopping potential. With what potential should a beam of electron be accelerated So that its wavelength becomes equal to $1.54A^{\large\circ}$

asked Feb 10, 2014 by sharmaaparna1

1 answer

De-Broglie proposed dual nature for electron by putting his famous equation $\lambda = \large\frac{h}{mu}$. Later on Heisenburg proposed uncertainity principle as $\bigtriangleup p .\bigtriangleup x \geq \large\frac{h}{2}(h = \large\frac{h}{2\pi})$ . On the contrary particle nature of electron was established on the basis of photoelectric effect. When a photon strikes the metal surface , it gives up its energy to the electron. Part of this energy (say w) is used by the electron to escape from the metal and the remaining imparts the kinetic energy $\large\frac{1}{2}mu^2$ to the photoelectron. The potential applied on the surface to reduce the velocity of photoelectron to zero is known as stopping potential . The wavelength of helium atom whose speed is equal to its rms speed at $27^{\large\circ}$ C

asked Feb 9, 2014 by sharmaaparna1

1 answer

De-Broglie proposed dual nature for electron by putting his famous equation $\lambda = \large\frac{h}{mu}$. Later on Heisenburg proposed uncertainity principle as $\bigtriangleup p .\bigtriangleup x \geq \large\frac{h}{2}(h = \large\frac{h}{2\pi})$ . On the contrary particle nature of electron was established on the basis of photoelectric effect. When a photon strikes the metal surface , it gives up its energy to the electron. Part of this energy (say w) is used by the electron to escape from the metal and the remaining imparts the kinetic energy $\large\frac{1}{2}mu^2$ to the photoelectron. The potential applied on the surface to reduce the velocity of photoelectron to zero is known as stopping potential. With what velocity must an electron travel so that its momentum is equal to that of photon of wavelength of $\lambda = 5200A^{\large\circ}$

asked Feb 9, 2014 by sharmaaparna1

1 answer

An oil drop has $-6.39\times10^{-19}$ coulomb charge .The number of electrons in this oil drop is

asked Feb 9, 2014 by sharmaaparna1

1 answer

The electrons in a poly-electronic atom are filled one by one in order of increasing energy level.The energy of sub shells and orientation of orbitals depends upon the values of three quantum numbers(i.e n,l and m respectively ) derived from Schrodinger wave equation. The different orbitals of subshells however possess same energy level and are called degenerate orbitals but their energy level changes in presence of magnetic field and the orbitals are non-degenerate. A spectral line is noticed if an electron jumps from one level to other. The paramagnetic nature of element is due to the presence of unpaired electron. The number of spherical and angular nodes in 2p orbital are:

asked Feb 9, 2014 by sharmaaparna1

1 answer

The electrons in a poly-electronic atom are filled one by one in order of increasing energy level.The energy of sub shells and orientation of orbitals depends upon the values of three quantum numbers(i.e n,l and m respectively ) derived from Schrodinger wave equation. The different orbitals of subshells however possess same energy level and are called degenerate orbitals but their energy level changes in presence of magnetic field and the orbitals are non-degenerate. A spectral line is noticed if an electron jumps from one level to other. The paramagnetic nature of element is due to the presence of unpaired electron. The total Magnetic momentum of $Ni^{2+}$ ion is....

asked Feb 9, 2014 by sharmaaparna1

1 answer

The electrons in a poly-electronic atom are filled one by one in order of increasing energy level.The energy of sub shells and orientation of orbitals depends upon the values of three quantum numbers(i.e n,l and m respectively ) derived from Schrodinger wave equation. The different orbitals of subshells however possess same energy level and are called degenerate orbitals but their energy level changes in presence of magnetic field and the orbitals are non-degenerate. A spectral line is noticed if an electron jumps from one level to other. The paramagnetic nature of element is due to the presence of unpaired electron. Which in each pair is most stable ion: $Cu^+ or Cu^{2+} and Fe^{2+} or Fe^{3+}$

asked Feb 9, 2014 by sharmaaparna1

1 answer

Rutherford proposed the atomic model after his most striking experiment on $\alpha$ – scattering leading to discovery of nucleus. Bohr later on modified the atomic model on the basis of Planck’s quantum theory of light and proposed the concept of stationary circular orbits of quantised energy $\large\frac{nh}{2\pi}$. The collection of fine lines in line spectrum led Sommerfeld to gave the idea of elliptical orbits. He successfully explained the existence of subshells and their number in a shell. The angular momentum of subshells was propped as $\sqrt{l(l+1}\times\large\frac{h}{2\pi}$. The emission of a spectral line in atomic spectra was supposed to be due to the jump of electron from one energy level to other. An oil drop has $-6.39\times10^{-19}$ coulomb charge. The number of electrons in this oil drop is

asked Feb 8, 2014 by sharmaaparna1

1 answer

Rutherford proposed the atomic model after his most striking experiment on $\alpha$ – scattering leading to discovery of nucleus. Bohr later on modified the atomic model on the basis of Planck’s quantum theory of light and proposed the concept of stationary circular orbits of quantised energy $\large\frac{nh}{2\pi}$. The collection of fine lines in line spectrum led Sommerfeld to gave the idea of elliptical orbits. He successfully explained the existence of subshells and their number in a shell. The angular momentum of subshells was propped as $\sqrt{l(l+1}\times\large\frac{h}{2\pi}$. The emission of a spectral line in atomic spectra was supposed to be due to the jump of electron from one energy level to other. An oxide on N has vapour density 46. The total number of electrons in 92g of it are:

asked Feb 8, 2014 by sharmaaparna1

1 answer

Rutherford proposed the atomic model after his most striking experiment on $\alpha$ – scattering leading to discovery of nucleus. Bohr later on modified the atomic model on the basis of Planck’s quantum theory of light and proposed the concept of stationary circular orbits of quantised energy $\large\frac{nh}{2\pi}$. The collection of fine lines in line spectrum led Sommerfeld to gave the idea of elliptical orbits. He successfully explained the existence of subshells and their number in a shell. The angular momentum of subshells was propped as $\sqrt{l(l+1}\times\large\frac{h}{2\pi}$. The emission of a spectral line in atomic spectra was supposed to be due to the jump of electron from one energy level to other. What is the minimum energy given out when an electron jumps from one orbit to other form.

asked Feb 8, 2014 by sharmaaparna1

1 answer

Rutherford proposed the atomic model after his most striking experiment on $\alpha$ – scattering leading to discovery of nucleus. Bohr later on modified the atomic model on the basis of Planck’s quantum theory of light and proposed the concept of stationary circular orbits of quantised energy $\large\frac{nh}{2\pi}$. The collection of fine lines in line spectrum led Sommerfeld to gave the idea of elliptical orbits. He successfully explained the existence of subshells and their number in a shell. The angular momentum of subshells was propped as $\sqrt{l(l+1}\times\large\frac{h}{2\pi}$. The emission of a spectral line in atomic spectra was supposed to be due to the jump of electron from one energy level to other. Calculate the total number of fundamental particles in $^{14}_6C$ is

asked Feb 8, 2014 by sharmaaparna1

1 answer

Rutherford proposed the atomic model after his most striking experiment on $\alpha$ – scattering leading to discovery of nucleus. Bohr later on modified the atomic model on the basis of Planck’s quantum theory of light and proposed the concept of stationary circular orbits of quantised energy $\large\frac{nh}{2\pi}$. The collection of fine lines in line spectrum led Sommerfeld to gave the idea of elliptical orbits. He successfully explained the existence of subshells and their number in a shell. The angular momentum of subshells was propped as $\sqrt{l(l+1}\times\large\frac{h}{2\pi}$. The emission of a spectral line in atomic spectra was supposed to be due to the jump of electron from one energy level to other. Calculate the Non-directional orbital.

asked Feb 8, 2014 by sharmaaparna1

1 answer

Rutherford proposed the atomic model after his most striking experiment on $\alpha$ – scattering leading to discovery of nucleus. Bohr later on modified the atomic model on the basis of Planck’s quantum theory of light and proposed the concept of stationary circular orbits of quantised energy $\large\frac{nh}{2\pi}$. The collection of fine lines in line spectrum led Sommerfeld to gave the idea of elliptical orbits. He successfully explained the existence of subshells and their number in a shell. The angular momentum of subshells was propped as $\sqrt{l(l+1}\times\large\frac{h}{2\pi}$. The emission of a spectral line in atomic spectra was supposed to be due to the jump of electron from one energy level to other. Then the volume occupied by the nucleus is about .....times of volume of atom.

asked Feb 8, 2014 by sharmaaparna1

1 answer

Rutherford proposed the atomic model after his most striking experiment on $\alpha$– scattering leading to discovery of nucleus. Bohr later on modified the atomic model on the basis of Planck’s quantum theory of light and proposed the concept of stationary circular orbits of quantised energy $\large\frac{nh}{2\pi}$. The collection of fine lines in line spectrum led Sommerfeld to gave the idea of elliptical orbits. He successfully explained the existence of subshells and their number in a shell. The angular momentum of subshells was propped as $\sqrt{l(l+1}\times\large\frac{h}{2\pi}$. The emission of a spectral line in atomic spectra was supposed to be due to the jump of electron from one energy level to other. Calculate the angular momentum of electron in 2p orbital is

asked Feb 8, 2014 by sharmaaparna1

1 answer

Calculate the shortest and longest wavelength in H spectrum of Lyman series. $R_H = 109678 cm^{-1}$

asked Feb 7, 2014 by sharmaaparna1

1 answer

If the radius of first Bohr orbit of hydrogen atom is 'x' then de Broglie wavelength of electron in $3^{rd}$ Orbit is nearly

asked Feb 7, 2014 by sharmaaparna1

1 answer

How many times does light travel faster in vaccum than an electron in Bohr first orbit of hydrogen atom?

asked Feb 7, 2014 by sharmaaparna1

1 answer

Imagine an atom made up of proton and a hypothetical particle of double the mass of electron but having the same charge as the electron . Apply the Bohr's atomic model and consider all possible transitions of this hypothetical particle to the first excited level. The largest wavelength photon that will be emitted has wavelength $\lambda$ (given in terms of the Rydberg constant R for the hydrogen atom) equal to.

asked Feb 7, 2014 by sharmaaparna1

1 answer

The total energy of the electron of H-atom in the Second quantum State is $E_2$. The total energy of the ${He^+}$ atom in the third quantum state is

asked Feb 7, 2014 by sharmaaparna1

1 answer

When a hydrogen atom emits a photon of energy 12.1eV, the orbital angular momentum changes by

asked Feb 7, 2014 by sharmaaparna1

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What is the ratio of the Rydberg constant for helium to hydrogen atom?

asked Feb 6, 2014 by sharmaaparna1

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What is energy per mol of photons of FM radiowaves with V=102.5 MHZ ?

asked Feb 6, 2014 by sharmaaparna1

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The dissociation energy of $H_2$ is 430.53KJ. If $H_2$ is exposed to light energy of wavelength 253.7 nm , what $\%$ of light energy will be converted into kinetic energy?

asked Feb 6, 2014 by sharmaaparna1

1 answer

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