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During winters, moisture condness in the...

During winters, moisture condness in the form of dew and can be seen on plant leaves and grass. The entropy of the system in such cases decreases as liquids posses lesser disorder compared to gases. With prefrence to the second law, which statement is correct, for the above proces?

A

The randomnes of the unierse decreases.

B

The randomnesof the surroundings decreases.

C

Increases is randomne of surrroundings equals the decreases in randomnes of system.

D

The increase in randomnes of the surrounding is greater as compared to the decrease in randomnes of the system.

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The correct Answer is:
D
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During winters, moisture condenses in the from of dew and can be seen on plant leaves and grass. The entropy of the system in such cases decreases as liquids process lesser disorder as compared to gases. With reference to the second law, which statement is correct. for the above process?

If a system at equilibrium is subjected to a change of any one of the factors such as concentration , pressure or temperature, the system adjusts itself in such a way so as to minimise the effect of that change. Effect of change in concentration on equilibrium: As we add or remove reactant (or product) the ratio of equilibrium concentratio become 'Q' (reaction quotient) and depending upon. QltK : equilibrium will shift ihn forward direction QgtK equilibrium will shift in backward direction Effect of change in pressure : If a system in equilibrium consists of gases, then the concentrations of all the components can be altered by changing the pressure. When the pressure on the system is increased, then equilibrium will shift in the direction in which there is decrease in number of moles i.e., towards the direction in which there is decrease in volume. Effect of change in pressure on melting point : There are two rypes of solids : Solids whose volume decreases on melting, e.g., ice, diamond, carborundum, magnesium nitride and quartz. Solid (higher volume) hArr Liquid (higher volume) The process of melting is facillitated at high pressure, thus melting point is lowered. Solid whose volume increase on melting, e.g., Fe, Cu, Ag, Au, etc. Solid (lower volume) hArr Liquid (higher volume) In this case the process of melring becomes difficult at high pressure, thuse melting point becomes high. Solubility of substances : When solid substance are dissolved in water, either heat is evolved. for endothermic solubility process solubility increase with increase in temperature. For exothemic solubility decrease with increase in temperature. Solubility of gases in liquids : when a gas dissolves in liquid, there is decreases in voolume. Thus increase of pressure will faavour the dissolution of gas in liquid. Effect of temperature : For endotherimic reacrtion as temperature increases reaction shift in backward direction Fe(l)hArrFe(s) Above equilibrium is favaured at :

Work done by the system in isothermal reversible process is w_(rev.)= -2.303 nRT "log"(V_(2))/(V_(1)) . Also in case of adiabatic reversible process work done by the system is given by: w_(rev.) = (nR)/(gamma -1) [T_2 - T_1] . During expansion disorder increases and the increase in disorder is expressed in terms of change in entropy DeltaS = q_(rev.)/T . The entropy changes also occurs during transformation of one state to other end expressed as DeltaS = DeltaH/T . Both entropy and enthalpy changes obtained for a process were taken as a measure of spontaniety of process but finally it was recommended that decrease in free energy is responsible for spontaniety and DeltaG=DeltaH - T DeltaS . Which statements are correct? (1) The expansion work for a gas into a vacuum is equal to zero. (2) 1 mole of a gas occupying 3 litre volume on expanding to 15 litre at constant pressure of 1atm does expansion work 1.215 kJ . (3) The maximum work done during expansion of 16gO_2 at 300K from 5dm^3 to 25 dm^3 is 2.01 kJ . (4) The DeltaS for S to L is almost negligible in comparision to DeltaS for L to G . (5) DeltaS = 2.303 nR "log"(V_(2))/(V_(1)). (at constant T )

Free enegry , G = H - TS , is state function that indicates whther a reaction is spontaneous or non-spontaneous. If you think of TS as the part of the system's enegry that is disordered already, then (H -TS) is the part of the system's energy that is still ordered and therefore free to cause spontaneous change by becoming disordered. Also, DeltaG = DeltaH - T DeltaS From the second law of thermodynamics, a reaction is spontaneous if Delta_("total")S is positive, non-spontaneous if Delta_("total")S is negative, and at equilibrium if Delta_('total")S is zero. Since, -T DeltaS = DeltaG and since DeltaG and DeltaS have opposite sings, we can restate the thermodynamic criterion for the spontaneity of a reaction carried out a constant temperature and pressure. IF DeltaG lt 0 , the reaction is spontaneous. If DeltaG gt 0 , the reaction is non-spontaneous. If DeltaG = 0 , the reaction is at equilibrium. Read the above paragraph carefully and answer the following questions based on the above comprehension. For the spontaneity of a reaction, which statement is true?

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