# The mass of air in the pressurised air tank

• Gregs6799
In summary: You are still making mistakes. You forgot to divide the absolute pressure (270) by the atmospheric pressure (101,325). You also forgot to divide the volume (450) by the pressure (270). 437,955,831 / 270 = 1,429,312,000You are still making mistakes. You forgot to divide the absolute pressure (270) by the atmospheric pressure (101,325). You also forgot to divide the volume (450) by the pressure (270). 437,955,831 / 270 = 1,429,312,000
Gregs6799

## Homework Statement

A pressurised air tank supplies compressed air to an air engine. When the air engine is not running the absolute pressure in the tank is 300 bar and the temperature of the air is 60°C.

Calculate:
(a) The temperature of the air in the high pressure air tank when the air engine starts and the absolute pressure in the tank drops to 270 bar. Volume remains constant.

(b) The mass of air in the pressurised air tank using the temperature and pressure from part 1 (a).

M = pV / RT [/B]
p = 270
V = 450
R = 8.314
T = 299.7

## The Attempt at a Solution

(a) is fine just need help with (b)
I found the temperature to be 26.7 for the answer to (a) and added 273 to covert into kelvins (299.7)
270 x 450 / 8.314 x 299.7 = 4,379,787 which seems way too high.

How do I convert this into a 3 figure answer from mol mass to j/kgk or can the mass be that high?
[/B]

You need to do the arithmetic correctly.

I've tried 4,379 / 273 = 16.04, would that be any closer?
Or am I confusing temperatures with weight units?

Gregs6799 said:
270 x 450 / 8.314 x 299.7 = 4,379,787

As Chestermiller was trying to get you to notice, you calculated incorrectly. The right side does not equal the left side. I believe you forgot that the 299.7 is in the denominator.

Chestermiller
I didn't realize that both sides had to equal each other.
Could you point me in the right direction with the formula for the mass, I believe it to be pV / RT?

Gregs6799 said:
I didn't realize that both sides had to equal each other.
Could you point me in the right direction with the formula for the mass, I believe it to be pV / RT?
You are misunderstanding. You made a calculation error. You said 2+2 = 17. If you type what you wrote into a calculator exactly the way you wrote it you get your 4379787. That’s because the two numbers in the denominator should be in parentheses. Your calculator doesn’t know what you mean and it multiplies by 299.7 instead of dividing by 299.7 making your answer wrong by 299.7^2

Even when you get the arithmetic right, it's still wrong. What are the units of P, V, R and T? Are they consistent? What are the units of your answer?
This is an excellent example of the rule that you should NEVER simply plug numbers into an equation without thinking about units. Get into the habit of always including the units of every quantity; it will save you a lot of mistakes.
E.g. P atm * V L/(R L-atm/mol/K * T K) = (PV/RT) mol
The answer to a question that asks for mass can never be a bare number. It must have units - is it kg, g, lb, amu etc?
And no, mass is not pV/RT. What is the basic ideal gas law?

Cutter Ketch and Chestermiller
Cutter Ketch & mjc 123 thanks for your replies.
The Ideal Gas Law. The volume (V) occupied by n moles of any gas has a pressure (P) at temperature (T) in Kelvin. The relationship for these variables, P V = n R T, where R is known as the gas constant, is called the ideal gas law.
I'm very new to physics, but I've found the mols to be 4,379787 from 270bar x 450l / 8.314J·K-1·mol- x 299.7K
which can't be right.
But I also tried 270bar x 450l / 8.314J·K-1·mol- / 299.7K = 48.76kg which sounds like the better answer but I know I've left out the air value 28.96Mr (g/mol) from the equation.
So I tried 28.96Mr x 8.314J·K-1·mol- x 299.7K / 270bar x 450l = 120,266
My tutor isn't much help and my notes don't seem cover everything asked in the assessment, but I'm probably going to struggle to understand a lot of what your explaining but do appreciate your help.

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The units of R have to be consistent with the units of your other parameters. Are they?

You're just guessing. Don't guess. Think.
You know that PV/RT gives you the number of moles (though you got both the calculation and the units wrong). How do you get from the number of moles to the mass?
And you really MUST get the units right. bar*L/(J/mol/K*K) doesn't give you moles. It gives you mol*bar*L/J. You must use consistent units. My preference is to convert everything into SI units before applying the equation, but you can use other units if you are consistent. There is a value of R in L*atm/mol/K - google "gas constant" and see if you can find it.

Chestermiller
I found the value 0.082057 L atm mol-1 K-1 instead of 8.314
I've converted 270 bar to 266.469 atm
266.469 x 450 / 0.082057 x 299.7 = 437,955,831
Number of moles = 437,955,831

Gregs6799 said:
I found the value 0.082057 L atm mol-1 K-1 instead of 8.314
I've converted 270 bar to 266.469 atm
266.469 x 450 / 0.082057 x 299.7 = 437,955,831
Number of moles = 437,955,831
You still messed up the arithmetic (making the same mistake as before). Also, I assume the volume is 450 liters and not 450 m^3?

It's good also to get into the habit of writing parentheses when appropriate, e.g.
266.469 x 450 / (0.082057 x 299.7)
Otherwise you will often make mistakes. Make sure, too, that you know how to enter an expression like that into your calculator or spreadsheet so that it does the right calculation.

The volume is 450 litres (not m^3) and I don't know where I'm going wrong with the arithmetic, I've tried the different values for R as mjc123 asked me too, and converted 270 bar into atm.
I hope your not sick of me getting it wrong but its all new to me.

Okay, do it in two steps. Calculate X = P x V, and Y = R x T. Then divide X by Y. Can you see how you weren't doing that?

(0.082057 x 299.7) / 266.469 x 450 = 41.530
I understand to do the bracket sum first now.

You are still making exactly the same error, but this time with the expression the wrong way up! I said divide X by Y; that means X/Y, not Y/X. (Perhaps I should have put brackets round the numerator as well, but I didn't think you were going to put it on the bottom!) You need to calculate
(266.469 x 450) / (0.082057 x 299.7)

Chestermiller
I did X / Y and I'm getting 121,500 / 2,491.7058 = 48.761kg which sounds right
266.469 x 450 / 0.082057 x 299.7 = 437,955,831

You have used the value 8.314 for R instead of 0.082!
And for the umpteenth time, PV/RT does NOT give you kg! What does it give you?

Mol Mass

No it does not! If pV = nRT, what is PV/RT?

$$n=\frac{PV}{RT}=\frac{(266.49)(450)}{(0.082157)(299.7)}=4876\ gm-moles$$
What is the molar mass of air?
How many grams of air is 4876 gm-moles?
How many kg is that?

Molar mass of air = 28.96
4876 = 87841.1g or 87.84kg
But I get 437,457,232 from your equation.

Gregs6799 said:
Molar mass of air = 28.96
4876 = 87841.1g or 87.84kg
But I get 437,457,232 from your equation.
You need to learn how to do arithmetic. My equation does not give that. You multiplied by 299.7 rather than dividing by it. And your multiplication of 28.96 times 4876 should not give 87841.1.

Yeah I multiplied the 299.7 and dividing it got me to your answer.
I didn't multiply 28.96 by 4876, I had to google the grams of 4876 moles and I found 87841.1g and take 87.84kg to be my answer.

Gregs6799 said:
Yeah I multiplied the 299.7 and dividing it got me to your answer.
I didn't multiply 28.96 by 4876, I had to google the grams of 4876 moles and I found 87841.1g and take 87.84kg to be my answer.
That would be the result if you had 4876 moles of water (of molar mass 18). But you have 4876 moles of air (of molar mass 28.96).

4879moles x 28.96 = 141,295.85

141,295.85 / 4879 = 28.96

Molecular mass = 28.96kg

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Gregs6799 said:
4879moles x 28.96 = 141,295.85

141,295.85 / 4879 = 28.96

Molecular mass = 28.96kg
What is it in kg?

141,295.85g so 141kg which again seems so high

Gregs6799 said:
141,295.85g so 141kg which again seems so high
Really? In a tank with a (large) volume of 0.45 m^3 and a (high) pressure of nearly 300 atm, you feel that that seems high?

It's just the picture I have makes it look fairly small, but with the equations I've done it has to be the correct answer.
Sorry it's taken so long but in my notes there's no examples with different values to compare and my tutor isn't easy to get hold of.
Thanks again.

Gregs6799 said:
It's just the picture I have makes it look fairly small, but with the equations I've done it has to be the correct answer.
Sorry it's taken so long but in my notes there's no examples with different values to compare and my tutor isn't easy to get hold of.
Thanks again.
Most of your difficulty has not been with the physics of the problem. It has been with your difficulty with mathematics.

## What is the mass of air in the pressurised air tank?

The mass of air in a pressurized air tank depends on the volume of the tank and the pressure of the air inside. The higher the pressure and volume, the greater the mass of air. This can be calculated using the ideal gas law, which states that the mass of a gas is directly proportional to its pressure and volume.

## How is the mass of air in the pressurised air tank measured?

The mass of air in a pressurized air tank can be measured using a scale or balance. The tank should be weighed when it is empty and then again when it is filled with air at a given pressure. The difference in weight will give the mass of air in the tank.

## Does the temperature affect the mass of air in the pressurised air tank?

Yes, the temperature does affect the mass of air in the pressurized air tank. As the temperature increases, the molecules of air gain more kinetic energy and move faster, resulting in an increase in mass. This can be accounted for by using the ideal gas law, which includes temperature as a variable.

## Can the mass of air in the pressurised air tank change over time?

Yes, the mass of air in a pressurized air tank can change over time. This can be due to a variety of factors such as leaks, changes in temperature, or changes in pressure. It is important to regularly check and maintain the pressure and volume of the tank to ensure the mass of air remains consistent.

## How does the mass of air in the pressurised air tank affect its performance?

The mass of air in the pressurized air tank directly affects its performance. A higher mass of air means there is more air available to be released, resulting in a stronger and longer-lasting burst of air. However, a heavier tank may also be more difficult to transport and may require more energy to pressurize.

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