It is desired to obtain A volume of 1.00L of nitrogen at 100°C and 640mmHg. How many grams of nitrogen would be required?

Mass of Nitrogen is 0.378 g.

Explanation:

We have to find the number of moles of nitrogen by using the ideal gas equation, then from the moles we have to find the mass in grams using its molar mass.

PV = nRT

We have to use,

Pressure = 640 mm Hg = 0.84 atm

Volume = 1 L

Temperature = 100° C + 273 = 373 K

R = gas constant = 0.08205 L atm mol⁻¹K⁻¹

n =

 =

= 0.027 moles

Mass = moles × molar mass

        = 0.027 ×14 g/mol = 0.378 g

So the mass of nitrogen is 0.378 g.

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in molecule of water there are dipole-dipole forces between negatively charged oxygen from one molecule of water and positively charger hydrogen of another molecule of water.

hydrogen bond is an electrostatic attraction between two polar groups that occurs when a hydrogen atom (h), covalently bound to a highly electronegative atom such as flourine (f), oxygen (o) and nitrogen (n) atoms.