Answer to Question #210850 in Physical Chemistry for pesky

Question

1. 1 mole of an ideal gas is allowed to expand against a piston that supports 0.4atm. The initial pressure was 10atm and final pressure is 0.4atms, the temperature being kept constant at 0oC. 

(a) How much work is done by the gas during the expansion? 

(b) What is the change in internal energy and in the enthalpy of the gas

(c) How much heat is absorbed?

2.  One mole of gas is allowed to expand reversibly i.e. against confining pressure that is at all times infinitesimally less than the gas pressure, from an initial pressure of 10 atm to a final pressure of 0.4 atm, the temperature being kept constant at 00 C 

a.   Calculate how much work is done by the gas 

b.   Calculate the change in initial energy and enthalpy 

c.  Calculate how much heat is absorbed

(Useful constants: 1 atm = 101325Nm-2; R = 8.314JK-1mol-1; 1 Cal = 4.184J)

Answer 1

1.a) 567J

b)Change in internal energy=-364kJ/mol

c) Heat absorbed =+34kJ/mol

2.a) 567J

b)Change in internal energy=-364kJ/mol

c) Heat absorbed =+34kJ/mol