1) 0.50 mol of an ideal gas is expand isothermally against constant pressure of
ID: 891529 • Letter: 1
Question
1) 0.50 mol of an ideal gas is expand isothermally against constant pressure of 2.0 atm from 1.0 L to 5.0 L . After expansion, the gas is in equilibrium with its surrounding . Calculate the values of ds( system ), ds ( surrounding ) and ds ( universe )?2) the molar heat of vaporization of ethanol is 39.3 KJ/ mol, and the boiling point of ethanol is 78.3C. Calculate the value of ds ( vap ) for vaporization of 0.50 mol of ethanol?
3) the heat capacity of chronic gas is given by Cp= ( 31.00 + 0.008T ) J/mol K. Calculate the entropy change when 2 miles of gas are heated from 300 to 400 K at constant pressure ?
4) the heat capacity of hydrogen gas is given by Cp= ( 1.554+0.0022T) Jmol k . Calculate the entropy changes for system, surrounding,and universe for the a) reversible heating, b) irreversible heating of 1.0 mol of hydrogen from 300 to 600 K ? ( Assume the surrounding to be 600 for b ) 1) 0.50 mol of an ideal gas is expand isothermally against constant pressure of 2.0 atm from 1.0 L to 5.0 L . After expansion, the gas is in equilibrium with its surrounding . Calculate the values of ds( system ), ds ( surrounding ) and ds ( universe )?
2) the molar heat of vaporization of ethanol is 39.3 KJ/ mol, and the boiling point of ethanol is 78.3C. Calculate the value of ds ( vap ) for vaporization of 0.50 mol of ethanol?
3) the heat capacity of chronic gas is given by Cp= ( 31.00 + 0.008T ) J/mol K. Calculate the entropy change when 2 miles of gas are heated from 300 to 400 K at constant pressure ?
4) the heat capacity of hydrogen gas is given by Cp= ( 1.554+0.0022T) Jmol k . Calculate the entropy changes for system, surrounding,and universe for the a) reversible heating, b) irreversible heating of 1.0 mol of hydrogen from 300 to 600 K ? ( Assume the surrounding to be 600 for b )
2) the molar heat of vaporization of ethanol is 39.3 KJ/ mol, and the boiling point of ethanol is 78.3C. Calculate the value of ds ( vap ) for vaporization of 0.50 mol of ethanol?
3) the heat capacity of chronic gas is given by Cp= ( 31.00 + 0.008T ) J/mol K. Calculate the entropy change when 2 miles of gas are heated from 300 to 400 K at constant pressure ?
4) the heat capacity of hydrogen gas is given by Cp= ( 1.554+0.0022T) Jmol k . Calculate the entropy changes for system, surrounding,and universe for the a) reversible heating, b) irreversible heating of 1.0 mol of hydrogen from 300 to 600 K ? ( Assume the surrounding to be 600 for b )
Explanation / Answer
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1)
Work done ,W = -P(Vf-Vi)
= - 2*(5-1)
= -8 atmL
= -8*101.3 J
= -810.4 J
Since T is constant,, delta U =0
delta U = Q+W
so,
Q = -W
= 810.4 J
use P*V=n*R*T to find T
2*5 = 0.5*0.0821*T
T= 243.6 K
ds(system) = Q/T
=810.4 /243.6
= 3.33 J/K
Q for surrounding = -Q for system
=-810.4 J
Since temperature is same for surrounding,T =243.6 K
ds(surrounding) = Q of surrounding/T
= -810.4 /243.6
= -3.33 J/K
ds universe = ds(system) + ds(surrounding)
= 3.33 J/K - 3.33 J/K
= 0
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