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For which set of ΔH^{• }and ΔS^{ }will the reaction be spontaneous only at high temperature
At high temperature, ΔG = ΔH  TΔS
Only, ΔH = +ve , ΔS = +ve, T = high
Reaction spontaneous, ΔG = ve
The final temperature of one mole of gas at 200 atm an d 19°C as it is forced through a porous plug to a final pressure of 0.95 atm is _______________ K( μ_{JT} = 0.150 k atm) (Round off to two decimal places).
A quantity of CH_{4} (g) at 298K is compressed reversibly and adiabatically from 50.0 bar to 200 bar. Assuming ideal behaviour. The value of final temperature of CH_{4} (g). (Take = 3R ) ______________ (answer should be an integer).
Hie change in entropy, when temperature is lower down to 1/8 of initial temperature at constant volume is
The change in enthalpy when 5 mole of liquid benzene transforms to the vapour state at its boiling temperature(90°C) and at 1 bar pressure is (ΔS_{V} = 87J K mol) _____________________KJ. (Round off to two decimal places).
A steam engine operates between 400K and 300K under higher pressure. The minimum amount of heat that must be with drawn from the hot reservoir to obtain 1000 J of work is
The change in entropy if one mole of S0_{2}(g) at 300K and 1.00 bar is heated to 1000K and its pressure is decreased to 0.010 bar. The molar heat InCorrect capacity of SC_{2}(g) to be
The change in entropy for the following transformation is respectively (+ indicates increases.  indicates decreases and 0 indicates no change)
(i) Change in entropy = positive
(ii) Change in entropy = negative
(iii) Change in entropy = positive
(iv) Change in entropy = zero
A gas obeys the equation P (V_{m } b) = RT. For this gas b = 0.0391 dm^{3 }mol^{1 }.The fugacity coefficient for the gas at 1000°C and 1000 atm is
The correct relation for ΔU in van der Waal gas (in isothermal variation ) is
is exothermic by 97030 J at 298K and 1 atm measured in a bomb calorimeter. The value of ΔH is
The ΔG_{mix} when 10 moles of Ne get mixed with 20 moles of equimolar mixture of He and Ne is ____________kJ.(Round off to one decimal place)
A system filled with 0.505 mol of gas contracts reversibly from 1L to 0.10 L at constant temperature at 5°C. It simultaneously loses 1270 J of heat. The ΔU is____________J. (Round off to nearest integer))
q = 1270J
Even through process is isothermal but overall ΔU change is not zero. So. applying first law
ΔU = q + w = 1270 + 2688 = 14187
The molar heat capacity at constant pressure of H_{2}O (g) at 1.00 atm is given by
Cp =30.54 + 10.3 x 10^{3} T
The change in entropy when 2.0 mole of water at 1.00 atm. The temperature of H_{2}O(g) is increased from 300K to 1000K is____________J K. (Round off to two decimal places)
The molecular partition function of a system is given by where the symbols have their usual meanings. The heat capacity at constant volume for this system is
1 mole of N_{2,} 2 mole of O_{2} and 1 mole of CO_{2} were mixed at 300K. The entropy of mixing is
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One mole of an ideal ga s C_{v} = 1.5 R at temperature 40 0K is com pressed from 2 atm to 3 atm by a reversible isothermal path. Subsequantly, it is expanded back to 2 atm by a reversible adiabatic path. The value of final state in litre is
Choose the correct option in the favour of exact differential
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