Two moles of an ideal gas initially at ${27}^0$C and one atmospheric pressure are compressed isothermally and reversibly till the final pressure of the gas is 10 atm.Calculate q,w and$∆U$  for the process.

n = 2 moles
P1= 1 atm P2 = 10 atm (compression )
T = 27 C = 300 K (Constant Temp) 
Isothermal Reversible process


Work done is given by 
W = 2.303nRT log(P2/P1)
W = 2.303 *2 * 8.314 *300 * log(10/1) = 2.303*2*8.314*300*1 = 11488.28 J 

Using FLOT( first law of thermodynamics)
del U = q + w
for isothermal proces U constant
so del U = 0
q = -W
q = -11488.28 J