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Edit View History Bookmarks Window Help a session masteringchemistry.com Chem& 161 Su 16 Section B Chapter 5 Homework Exercise 5.37 Resources previous l 19 of 30 I next Exercise 5.37 Part A What is the partial pressure of the hydrogen gas? The hydrogen gas formed in a chemical reaction is collected over water at 30.0 °C at a total pressure of 733 mmHg mm Hg Submit My Answers Give Up Part B If the total volume of gas collected is 723 mL what mass of hydrogen gas is collected? Submit My Answers Give Up Continue

Explanation / Answer

vapor pressure of water at 30 deg.c = 31.8 mm Hg

total presssure is given as =738 mmHg

partial pressure of hydrogen = total pressure- saturation pressure ( vapor pressure) at 30 deg.c = 738-31.8=706.2 mm Hg

given Volume of gas = 723 ml, =723/1000L= 0.723L, P= 706.2 mm Hg= 706.2/760 Atm=0.93 atm ( 1 atm= 760 mm Hg)

T= 30 deg.c = 30+273.15= 303.15 K, R= 0.0821 L.atm/mole.K

from PV= nRT, n= number of moles= PV/RT= 0.93*0.723/(0.0821*303.15)=0.027 moles of hydrogen

Mass of hydorgne= moles* Molecular weight= 0.027*2= 0.054 gms

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