# Homework Help: (Thermodynamics) A tank with water & air heated

1. Dec 11, 2015

### Baybora

1. The problem statement, all variables and given/known data
For a rigid, impervious, closed tank - The volume of tank is filled with 70% water and the rest is with air- The initial temperature of the tank is 20 °C, and the absolute pressure is 1 bar. - What would be the final pressure if we raise the temperature to 200 °C?

2. Relevant equations

3. The attempt at a solution
I tried finding some values at the water-vapour table but I just dont know what to do about it because I cant be sure if the water will become vapour or will stay in its liquid form. ANY help is appreciated

2. Dec 11, 2015

### PietKuip

Do not be afraid!
It is not dangerous to start calculating with an assumption that turns out to be wrong.
(The vessel will not explode, you won't get burns, the only risk is that you would have to try something else.)

3. Dec 11, 2015

### Baybora

The problem is that I cant even be sure of my assumption. How am i supposed to know if the water will stay liquid or will turn into gas?

4. Dec 11, 2015

### SteamKing

Staff Emeritus
Water can't stay liquid at 200° C unless the internal pressure in the tank is greater than the vapor pressure of water at that temp.

5. Dec 11, 2015

### Staff: Mentor

Are you currently learning how to use the Steam Tables in your course, or are you learning about the ideal gas law and vapor pressure?

Chet

6. Dec 11, 2015

### Baybora

Yes and any way to find out if it will or not?

7. Dec 11, 2015

### Baybora

Its a off course question, asked by mentor at a company. He said it has the same principle for calculations for extruders which contain screw and barrel. He has given me time for me to solve it until the end of 1st semester and said I could ask anybody if I cant make it myself. I asked it to my teacher but she didnt help at all not sure if she wants me to think, study and learn by myself or she also doesnt know it either. So its probably higher than thermodynamics 1 course

8. Dec 11, 2015

### Staff: Mentor

Take as a basis a 1 cubic meter tank (the actual volume you take doesn't matter). First focus on the initial conditions. What is the specific volume of liquid water at 20 C and 1 atm? What is the equilibrium vapor pressure of water at 20 C? What is the specific volume of saturated water vapor at 20 C? Based on these answers, what is the initial mass of liquid water in the tank? What is the initial mass of water vapor in the tank? What is the initial total mass of water in the tank. What is the partial pressure of air initially? How many moles of air are in the tank initially?

When you have the answers to these questions, let's see what you get.

Chet

9. Dec 11, 2015

### PietKuip

You know that by the outcome of the calculation. When you numbers are consistent, that is the answer.

The water does not "know" either.

10. Dec 11, 2015

### Staff: Mentor

If you know the total mass M of water in the tank, you let the final amount of water vapor be x and the final amount of liquid water be M-x. You then look up the specific volume of saturated liquid water at 200 C and the specific volume of saturated water vapor at 200 C. Then you solve for x under the constraint that the total volume of liquid water and water vapor must be equal to the volume of the tank.

Chet

11. Dec 11, 2015

### PietKuip

There is no need to solve for x. The only question is what the pressure will be.

If there is any water in the liquid phase, you just look at the vapor pressure curve.

12. Dec 11, 2015

### Staff: Mentor

Well, if there is a change in the volume of liquid, the volume of the air also changes, and this can affect the partial pressure of the air and total pressure.

13. Jan 11, 2016

### Baybora

Bump

14. Jan 11, 2016

### Baybora

Still looking for answers. Need help with the calculation part mostly

15. Jan 11, 2016

### Staff: Mentor

You still haven't answered my questions in posts #5 and #8. How are we supposed to help you if you don't answer our leading questions? I know you can answer the question in post #5, because it doesn't require any analysis.

16. Jan 11, 2016

### Baybora

and for your 8th post you already pointed out the fact that makes it very complicated and that doesnt give me a clue what are the constants in here. Everything in this system are effected by the parameters

17. Jan 11, 2016

### Staff: Mentor

OK. Let's do it without using the steam tables. Let's take as the basis of the calculations a tank with a volume of 1 cubic meter. That means that there is 0.7 cubic meters of liquid water plus 0.3 cubic meters of a gaseous mixture of air an water vapor at 20 C and 1 bar. The first step is to figure out the mass of water and the mass of air in the tank to start with (this won't change when the contents is heated)? Do you know how to figure this part out?

Chet

18. Jan 11, 2016

### Staff: Mentor

I expect you to look up the data asked for in post #8 on your own. This is what is required to start solving this problem. In real life, people don't spoon feed you data like they do in school. Welcome to the real world.

If you follow the steps I am leading you through, starting with the answers to the questions in post #8, I can guarantee you will get your answer. Otherwise, good luck.

Chet

19. Jan 12, 2016

### Baybora

Ok so the volume density of saturated water at 20 C is 0.001002 m^3/kg ( neglecting the small difference between compressed water at 20 C and 1 bar) and the volume density of air at 20 C and 1 bar is around 0,833 m^3 / kg

Assuming we have a 1 m^3 tank we have

0,7 / 0,001002 = 698,6 kg of water and
0,3 / 0,8333 = 0,36 kg of air in the tank

20. Jan 12, 2016

### PietKuip

Chestermiller already told you that the 0.3 m^3 also contains water. Yet you refuse to calculate how much.

21. Jan 12, 2016

### Staff: Mentor

Nice job. Your answer is close, but not quite. There is a small amount of water in the gas phase. It isn't very important at 20 C, but the amount of water in the gas phase will be important at 200 C. Would you prefer to neglect it and move on to 200 C, or would you rather get the practice accounting for the water vapor even at 20 C? It's your call.

Chet

22. Jan 12, 2016

### Baybora

I think we will have to assume that they are seperated as just liquid water and air with no water vapor because i couldn't find a way to find out the amount of water in air without a given humidity ratio or other info. That's why I think we should neglect it.

Here's one of the sites I have checked if I can calculate the water vapor in air.

http://home.howstuffworks.com/humidifier1.htm

There it says "At 20 C air can hold up to 18 grams of water" so we can just know the limits of contained vapor unless we are given a humidity ratio which in this case we aren't

23. Jan 12, 2016

### Staff: Mentor

The partial pressure of the water vapor in the head space is equal to the equilibrium vapor pressure of water at 20 C. In other words, the air above the liquid water in the closed container equilibrates with the liquid water and becomes saturated. So the relative humidity in the air in the head space is 100%. What is the equilibrium vapor pressure of water at 20 C?

24. Jan 12, 2016

### Baybora

17,535 mm Hg = 0,0233 bar

Source :

http://genchem.rutgers.edu/vpwater.html

25. Jan 12, 2016

### Staff: Mentor

Excellent. So the partial pressure of water vapor in the head space is 0.0233 bars, and the partial pressure of air in the head space is 0.9767 bars. That gives a total pressure of 1 bar. Using the ideal gas law, how many gram moles of water are there in 0.3 cubic meters of head space at a partial pressure of 0.0233 bars and a temperature of 293 K (20 C)? Using the ideal gas law, how many gram moles of air are there in 0.3 cubic meters of head space at a partial pressure of 0.9767 bars and a temperature of 293 K (20 C)? Based on this, what is the mass of the water in the head space? What is the mass of air in the head space? What is the total mass of water (liquid and vapor) in the container?