Recent questions tagged physical-chemistry

Calculate the density of $CO_2\; at \;100^{\large\circ}C$ and 800mm Hg pressure.

asked Feb 12, 2014 by sharmaaparna1

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Calculate the weight of $CH_4$ in a 9 litre cylinder at 16 atm and $27^{\large\circ}$ (R = 0.08 litre atm $K^{-1}$)

asked Feb 11, 2014 by sharmaaparna1

1 answer

Calculate the temperature at which 28g $N_2$ occupies a volume of 10 litres at 2.46 atm.

asked Feb 11, 2014 by sharmaaparna1

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Calculate the volume occupied by 7g $N_2$ at $27^{\large\circ}$ and 750mm of Hg.

asked Feb 11, 2014 by sharmaaparna1

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An iron cylinder contains helium at a pressure of 250 Kpa at 300K. The cylinder can withstand a pressure of $1\times10^6 Pa$ . The room in which cylinder is placed catches fire. Predict whether the cylinder will blow up before it melts or not . melting point of cylinder = 1800K

asked Feb 11, 2014 by sharmaaparna1

1 answer

The density of $3M$ solution of $Na_2S_2O_3$ is $1.25$ $g mL^{−1}$. Calculate the mole fraction of $Na_2S_2O_3$.

asked Feb 11, 2014 by sharmaaparna1

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The density of 3M solution of $Na_2S_2O_3$ is 1.25 g $mL^{-1}$ Calculate the $\%$ by weight of $Na_2S_2O_3$.

asked Feb 11, 2014 by sharmaaparna1

1 answer

$HNO_3$ used as a reagent has specific gravity of $1.42 mL^{-1}$ and contains $70\%$ by strength $HNO_3$. Calculate Volume of water required to make $1\;N$ solution from $2\; mL$ concentrated $HNO_3?\;(\text{Normality}_{HNO_3} = 15.78)$

asked Feb 11, 2014 by sharmaaparna1

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$HNO_3$ used as a reagent has specific gravity of $1.42 mL^{-1}$ and contains $70\%$ by strength $HNO_3$. Calculate Volume of acid that contains 63g pure acid.

asked Feb 11, 2014 by sharmaaparna1

1 answer

$HNO_3$ used as a reagent has specific gravity of $1.42 mL^{-1}$ and contains $70\%$ by strength $HNO_3$. Calculate Normality of acid

asked Feb 11, 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 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 . 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. 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

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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

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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

1 answer

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

Calculate the maximum wavelength in $A^{\large\circ}$ a photon that can initiate the reaction. $Cl_2(g)\rightarrow 2cl(g), \bigtriangleup H = 247$ KJ/mol

asked Feb 6, 2014 by sharmaaparna1

1 answer

Sodium atom emits light with a wavelength of 330nm when an electron moves from a 4p orbital to a 3s orbital. what is the energy difference between the orbitals in KJ/mol?

asked Feb 6, 2014 by sharmaaparna1

1 answer

An argon laser emits blue light with a wavelength of 488.0nm. How many photon are emitted by this laser in 2.00 sec,operating a power of 515 milliwatts?(one watt = 1J$S^{-1}$)

asked Feb 6, 2014 by sharmaaparna1

1 answer

The energy required for the ionisation of a certain atom is $3.44\times10^{-18}J$. The absorption of a photon of unknown wavelength ionises the atom and ejects an electron with velocity $1.03\times10^6$ m/sec. Calculate the wavelength of the incident radiation.

asked Feb 5, 2014 by sharmaaparna1

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Calculate the wavelength of the first line and the series limit for the Lyman series for hydrogen.(Series limit is for the case when $n_2 = \infty)$

asked Feb 5, 2014 by sharmaaparna1

1 answer

An electron difraction experiment was performed with a beam of electrons accelerated by a potential difference of 10.0kV.What is the wavelength of the electron beam?(1KV = 1000V = 1000eV for the electron)

asked Feb 5, 2014 by sharmaaparna1

1 answer

A proton is accelerated to one tenth of the velocity of light. Suppose velocity can be measured with a precision of $\pm1\%$, what can be the uncertainity in its position?

asked Feb 5, 2014 by sharmaaparna1

1 answer

The speed of a certain proton is $4.5\times10^5m$ If the uncertainity is to be reduced to 0.01percent, what uncertainity in its location must be tolerated?

asked Feb 5, 2014 by sharmaaparna1

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Two particles A and B are in motion . if the wavelength associated with particle A is $5\times10^{-8}$m.Calculate the wavelength associated with particle B if its momentum is half of A.

asked Feb 5, 2014 by sharmaaparna1

1 answer

Calculate the wavelength of a helium atom whose speed is equal to root mean square speed at 293 K $(rms = \sqrt{3RT/m})$

asked Feb 4, 2014 by sharmaaparna1

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The wavelength of $\beta$ line of the Balmer Series is $4815 A^{\large\circ}$. What is the wavelength of $\alpha$ line of balmer Series of the same atom?

asked Feb 4, 2014 by sharmaaparna1

1 answer

AIR services on vividh Bharti is transmitted on 219m band.What is its transmission frequency in Hertz.

asked Feb 4, 2014 by sharmaaparna1

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A certain laser transition emits $6.37\times10^{15}$ quants per second per square meter. Calculate the power out put in joule per square metre per second. Given $\lambda$ = 632.8 nm.

asked Feb 4, 2014 by sharmaaparna1

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