Question

How many moles of gas are contained in a human breath that occupies 0.59L and has a pressure of 752 mm Hg at 36 Celsius?

Answer 1

INFORMATION:

We know that:

- the gas occupies 0.59L and has a pressure of 752 mm Hg at 36 Celsius

And we must find the number of moles of the gas

STEP BY STEP EXPLANATION:

To find the number of moles we need to use the ideal gas formula

$PV=nRT$

So, we must solve it for n

$n=\frac{PV}{RT}$

Now, the given information is

- Pressure (P) = 752 mmHg

- Volume (V) = 0.59 L

- Temperature (T) = 36°C

We can use R = 62.36 (mmHg * L)/(mol * K)

So, we must convert the temperature to K

$T=36\degree C+273.15K=309.15K$

Finally, replacing the values in the formula

$n=\frac{752mmHg\times0.59L}{62.36\frac{mmHg\cdot L}{mol\cdot K}\times309.15K}=0.0230mol$

0.0230 moles of gas are contained in a human breath that occupies 0.59L and has a pressure of 752 mm Hg at 36 Celsius.

ANSWER:

0.0230 mol