# PV diagrams monatomic ideal gas

## Homework Statement

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??

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Andrew Mason
Homework Helper

## Homework Statement

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??
I am having trouble following your reasoning.

First, why would W = Pi(Vf-Vi) if the pressure is constant at 2Pi for A-E?

Second, why would you use 3Pi for the E-D path? Is the pressure constant during that process? What is the relationship between P and V during an isothermal process?

AM