# How many kilograms of #O_2# gas are needed to give an oxygen pressure of 3.48 atm at 22°C?

Just to retire this question, let us specify a volume of

And we change this molar amount to a mass by:

I would like you to check my math. There are no refunds.

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To calculate the mass of O₂ gas, we can use the ideal gas law:

[PV = nRT]

Where:

- (P) is pressure (in atm),
- (V) is volume (in liters),
- (n) is the number of moles,
- (R) is the ideal gas constant (0.0821 L.atm/(mol.K)),
- (T) is temperature (in Kelvin).

Rearranging the formula to solve for moles ((n)):

[n = \frac{PV}{RT}]

To find the mass ((m)), we use the molar mass of O₂ (32 g/mol):

[m = n \times \text{molar mass of } O_2]

Given values:

- (P = 3.48 , \text{atm}),
- (V) is not provided,
- (R = 0.0821 , \text{L.atm/(mol.K)}),
- (T = 22°C = 295 , \text{K}).

If you have the volume ((V)), you can substitute these values into the formula to find the number of moles ((n)), and then calculate the mass ((m)).

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When evaluating a one-sided limit, you need to be careful when a quantity is approaching zero since its sign is different depending on which way it is approaching zero from. Let us look at some examples.

When evaluating a one-sided limit, you need to be careful when a quantity is approaching zero since its sign is different depending on which way it is approaching zero from. Let us look at some examples.

When evaluating a one-sided limit, you need to be careful when a quantity is approaching zero since its sign is different depending on which way it is approaching zero from. Let us look at some examples.

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