1. The problem statement, all variables and given/known data Suppose a monatomic ideal gas is changed from state A to state D by one of the processes shown on the PV diagram. (Let V1 = 4.80 L and P1 = 3.30 atm.) (a) Find the total work done on the gas if it follows the constant pressure path A−E followed by the constant temperature path E−D. (b)Calculate the total change in internal energy of the gas during the entire process. (c)Calculate the total heat flow into the gas 2. W=pi(vf-vi) (1.01e5)(3.3)(9.6-4.8)(.001)=1599.84 J (1.01e5)(6.6+3.3)(19.2-9.6)(.001)= 4799.5 J =6399 J Why is my work wrong??