How many moles of air are there in a 0.125 L Erlenmeyer flask if the pressure is 0.985 atm and the temperature is 20.0 oC?

Use ideal gas law and show work please. Thank you

The answer for the question is answered below.

Explanation:

Given:

volume (v) =0.125 L

Pressure (P) =0.985 atm

temperature (t) =20°C =20 + 273 =293 K

To solve:

no of moles (n)

We know;

According to the Avagadros law;

P × V = n × R × T

0.985 × 0.125 = n × 0.0821 × 293

0.123125= n × 24.0553

n =

n = 0.05 moles

0.05 moles of air is present i the Erlenmeyer flask

"you start with 15.67 g mgco3-xh2o, when heated and all the water is removed, you are left with 7.58 g mgco3 only.

therefore, you had 15.67 - 7.58 = 8.09g h2o  

moles of each :

7.58g mgco3 = ? moles = 7.58g / 83.4g/mole = 0.09moles  

8 09g h2o = ? moles = 8.09g / 18g/mole = 0.44moles  

molar ratio between the two by dividing both numbers by the smallest number :

0.09 / 0.09 = 1  

0.44 / 0.09 = 4.8  

mgco3-5h2o"