NEET Test Series from KOTA - 10 Papers In MS WORD
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CHXII05:SURFACE CHEMISTRY
320630
Which are not purely surface phenomena?
1 Adsorption, surface tension
2 Surface tension, viscosity
3 Adsorption, viscosity
4 Absorption, viscosity
Explanation:
Conceptual Questions
CHXII05:SURFACE CHEMISTRY
320631
The term 'sorption' stands for ....
1 Desorption
2 Absorption
3 Adsorption
4 Both absorption and adsorption
Explanation:
Sorption stands for both absorption and adsorption. We can understand this by using following figures
NCERT Exemplar
CHXII05:SURFACE CHEMISTRY
320632
During the adsorption of krypton on activated charcoal at low temperature,
1 \(\Delta \mathrm{H}>0\) and \(\Delta \mathrm{S} < 0\)
2 \(\Delta \mathrm{H} < 0\) and \(\Delta \mathrm{S} < 0\)
3 \(\Delta \mathrm{H}>0\) and \(\Delta \mathrm{S}>0\)
4 \(\Delta \mathrm{H} < 0\) and \(\Delta \mathrm{S}>0\)
Explanation:
Adsorption of krypton on activated charcoal at low temperature means it adsorbed by physisorption process. That means accumulation of gases on the surface of solid by weak van der Waal's forces. Adsorption is an exothermic process. So \(\Delta \mathrm{H}\) and \(\Delta \mathrm{S}\) are negative \((\Delta \mathrm{H} < 0, \Delta \mathrm{S} < 0)\) to this process due to freedom of movement of its molecules becomes restricted when gas is adsorbed.
KCET - 2010
CHXII05:SURFACE CHEMISTRY
320633
Which one of the following characteristics is associated with adsorption?
According to Gibbs-Helmholtz equation, \({\rm{\Delta G = \Delta H - T\Delta S}}\) Adsorption is spontaneous process, \({\rm{so}}\,\,{\rm{\Delta G = negative}}\) Adsorption is exothermic process, \({\rm{so}}\,\,{\rm{\Delta H = negative}}\) In adsorption entropy decreases, \({\rm{so}}\,\,{\rm{\Delta S = negative}}\) Therefore, \({\rm{\Delta G,\Delta H}}\,\,{\rm{and}}\,\,{\rm{\Delta S}}\) all are negative.
Sorption stands for both absorption and adsorption. We can understand this by using following figures
NCERT Exemplar
CHXII05:SURFACE CHEMISTRY
320632
During the adsorption of krypton on activated charcoal at low temperature,
1 \(\Delta \mathrm{H}>0\) and \(\Delta \mathrm{S} < 0\)
2 \(\Delta \mathrm{H} < 0\) and \(\Delta \mathrm{S} < 0\)
3 \(\Delta \mathrm{H}>0\) and \(\Delta \mathrm{S}>0\)
4 \(\Delta \mathrm{H} < 0\) and \(\Delta \mathrm{S}>0\)
Explanation:
Adsorption of krypton on activated charcoal at low temperature means it adsorbed by physisorption process. That means accumulation of gases on the surface of solid by weak van der Waal's forces. Adsorption is an exothermic process. So \(\Delta \mathrm{H}\) and \(\Delta \mathrm{S}\) are negative \((\Delta \mathrm{H} < 0, \Delta \mathrm{S} < 0)\) to this process due to freedom of movement of its molecules becomes restricted when gas is adsorbed.
KCET - 2010
CHXII05:SURFACE CHEMISTRY
320633
Which one of the following characteristics is associated with adsorption?
According to Gibbs-Helmholtz equation, \({\rm{\Delta G = \Delta H - T\Delta S}}\) Adsorption is spontaneous process, \({\rm{so}}\,\,{\rm{\Delta G = negative}}\) Adsorption is exothermic process, \({\rm{so}}\,\,{\rm{\Delta H = negative}}\) In adsorption entropy decreases, \({\rm{so}}\,\,{\rm{\Delta S = negative}}\) Therefore, \({\rm{\Delta G,\Delta H}}\,\,{\rm{and}}\,\,{\rm{\Delta S}}\) all are negative.
Sorption stands for both absorption and adsorption. We can understand this by using following figures
NCERT Exemplar
CHXII05:SURFACE CHEMISTRY
320632
During the adsorption of krypton on activated charcoal at low temperature,
1 \(\Delta \mathrm{H}>0\) and \(\Delta \mathrm{S} < 0\)
2 \(\Delta \mathrm{H} < 0\) and \(\Delta \mathrm{S} < 0\)
3 \(\Delta \mathrm{H}>0\) and \(\Delta \mathrm{S}>0\)
4 \(\Delta \mathrm{H} < 0\) and \(\Delta \mathrm{S}>0\)
Explanation:
Adsorption of krypton on activated charcoal at low temperature means it adsorbed by physisorption process. That means accumulation of gases on the surface of solid by weak van der Waal's forces. Adsorption is an exothermic process. So \(\Delta \mathrm{H}\) and \(\Delta \mathrm{S}\) are negative \((\Delta \mathrm{H} < 0, \Delta \mathrm{S} < 0)\) to this process due to freedom of movement of its molecules becomes restricted when gas is adsorbed.
KCET - 2010
CHXII05:SURFACE CHEMISTRY
320633
Which one of the following characteristics is associated with adsorption?
According to Gibbs-Helmholtz equation, \({\rm{\Delta G = \Delta H - T\Delta S}}\) Adsorption is spontaneous process, \({\rm{so}}\,\,{\rm{\Delta G = negative}}\) Adsorption is exothermic process, \({\rm{so}}\,\,{\rm{\Delta H = negative}}\) In adsorption entropy decreases, \({\rm{so}}\,\,{\rm{\Delta S = negative}}\) Therefore, \({\rm{\Delta G,\Delta H}}\,\,{\rm{and}}\,\,{\rm{\Delta S}}\) all are negative.
NEET Test Series from KOTA - 10 Papers In MS WORD
WhatsApp Here
CHXII05:SURFACE CHEMISTRY
320630
Which are not purely surface phenomena?
1 Adsorption, surface tension
2 Surface tension, viscosity
3 Adsorption, viscosity
4 Absorption, viscosity
Explanation:
Conceptual Questions
CHXII05:SURFACE CHEMISTRY
320631
The term 'sorption' stands for ....
1 Desorption
2 Absorption
3 Adsorption
4 Both absorption and adsorption
Explanation:
Sorption stands for both absorption and adsorption. We can understand this by using following figures
NCERT Exemplar
CHXII05:SURFACE CHEMISTRY
320632
During the adsorption of krypton on activated charcoal at low temperature,
1 \(\Delta \mathrm{H}>0\) and \(\Delta \mathrm{S} < 0\)
2 \(\Delta \mathrm{H} < 0\) and \(\Delta \mathrm{S} < 0\)
3 \(\Delta \mathrm{H}>0\) and \(\Delta \mathrm{S}>0\)
4 \(\Delta \mathrm{H} < 0\) and \(\Delta \mathrm{S}>0\)
Explanation:
Adsorption of krypton on activated charcoal at low temperature means it adsorbed by physisorption process. That means accumulation of gases on the surface of solid by weak van der Waal's forces. Adsorption is an exothermic process. So \(\Delta \mathrm{H}\) and \(\Delta \mathrm{S}\) are negative \((\Delta \mathrm{H} < 0, \Delta \mathrm{S} < 0)\) to this process due to freedom of movement of its molecules becomes restricted when gas is adsorbed.
KCET - 2010
CHXII05:SURFACE CHEMISTRY
320633
Which one of the following characteristics is associated with adsorption?
According to Gibbs-Helmholtz equation, \({\rm{\Delta G = \Delta H - T\Delta S}}\) Adsorption is spontaneous process, \({\rm{so}}\,\,{\rm{\Delta G = negative}}\) Adsorption is exothermic process, \({\rm{so}}\,\,{\rm{\Delta H = negative}}\) In adsorption entropy decreases, \({\rm{so}}\,\,{\rm{\Delta S = negative}}\) Therefore, \({\rm{\Delta G,\Delta H}}\,\,{\rm{and}}\,\,{\rm{\Delta S}}\) all are negative.
