A sample of exhaled air contains four gases with the following partial pressures

Question

A sample of exhaled air contains four gases with the following partial pressures: O_2 (126 mm Hg), H_2O (52 mm Hg), CO_2 (45 mm Hg), and N_2 (542 mm Hg). What is the total pressure of the sample? How many moles of gas are contained in a human breath that takes in 0.75 L of air at 1.0 atm pressure and 37 degree C? Compounds with strong intermolecular forces have high point points and low vapor pressure. Circle one: True False Melting is an exothermic process. Circle one: True False Glass is an example of an amorphous solid. Circle one: True False

Explanation / Answer

partial pressure represents the pressure exerted by the specific gas in the mixture.... so P total = sum of all the partial pressure of gases...

hence PT = 126 + 52 + 45 + 542

= 765 mm og Hg

2) using ideal gas equation

PV = nRT

or n = PV/RT

= (1 X 0.75) / (0.0821 X 310)

=0.03 mols

3) vapour pressure is th epressure exerted by the gaseous molecules onthe surface of the liquid .... since compounds with strong intermolecular forces are firmly holding other molecules ..hence amount of molecules escdaping the surgace of liquid will be less ....hence True

4) to melt ..we are doing a phase change ...which will require a certain amount of energy ...hence ..the melting point should be an endothermic process..hence False

5) glass is an amorphous solid because it doen;t have asharp melting point....hence True

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