Please help me solve this, I cannot get the correct answer Relatively easy

[sprinstess]

A cylinder contains oxygen gas at a pressure of 2.20 atm. The volume is 6.00L, and the temperature is 300K Assume that the oxygen may be treated as an ideal gas. The oxygen is carried through the following processes:
(1) Heated at constant pressure from the initial state (state 1) to state 2, which has 440 K
(2) Cooled at constant volume to 250K (state 3).
(3) Compressed at constant temperature to a volume of 6.00 L (state 4).
(4) Heated at constant volume to 300K, which takes the system back to state 1.


For the life of me I cannot figure this problem out.
I filled out the table, getting 1.) 2.2atm, 6L, 300k, 2.) 2.2atm, 8L, 440K, 3.) 1.375atm, 8L,250k, 4.) 1.833atm, 6L, 250K

I also calculated the number of moles using the PV=nRT with the initial information in the problem and got .5362

From this I followed the sheet that is given on exams and plugged in the correct formulas for constant V,P, and T. And for work for Constant Pressure, I changed the 2.2 atm to Pa (by multiplying 101,325*2.2) and changed the liters to m^3 by dividing them by 1000.

Anyways, for my Q values I got -2005.3677, 2115.726, 320.465, and -556.97775. When I input them in, it says that Q2 is not quite; however I have calculated it multiple times. Also, it says my work is incorrect for Part B, and I have also recalculated them several times and gotten relatively close values.

Any help is appreciated!

 

[anathema]

I understand your frustration with this problem. It can be challenging to keep track of all the variables and equations involved in thermodynamics calculations. However, let me try to break down the problem and provide some guidance.

First, let's review the ideal gas law: PV = nRT, where P is pressure, V is volume, n is the number of moles, R is the gas constant, and T is temperature. This law can be used to calculate any of these variables, as long as we have values for the other variables.

In this problem, we are given the initial state (state 1) of the oxygen gas, which is 2.20 atm, 6.00 L, and 300 K. From this information, we can calculate the number of moles of oxygen gas using the ideal gas law. You correctly calculated this as 0.5362 moles.

Next, we need to keep track of the changes in pressure, volume, and temperature as the oxygen gas goes through the different processes. Let's go through each step one by one.

(1) In this step, the oxygen gas is heated at constant pressure from 300 K to 440 K. This means that the pressure (2.20 atm) and volume (6.00 L) remain constant, while the temperature changes. Using the ideal gas law, we can calculate the final number of moles of oxygen gas at state 2 as 0.6461 moles.

(2) In this step, the oxygen gas is cooled at constant volume from 440 K to 250 K. This means that the volume (6.00 L) remains constant, while the pressure and temperature change. Using the ideal gas law, we can calculate the final pressure at state 3 as 1.375 atm.

(3) In this step, the oxygen gas is compressed at constant temperature (250 K) to a volume of 6.00 L. This means that the temperature remains constant, while the pressure and volume change. Using the ideal gas law, we can calculate the final pressure at state 4 as 1.833 atm.

(4) In this final step, the oxygen gas is heated at constant volume from 250 K back to 300 K. This means that the volume (6.00 L) remains constant, while the pressure and temperature change. Using the ideal gas law,