
#1
Oct1407, 09:11 PM

P: 62

1. The problem statement, all variables and given/known data
A sample was collected into a 1.25L tank at 752 mm Hg and analyzed. The analysis showed 92% CO2, 3.6% NO, 1.2% SO2, and 4.1% H2O by mass(key word mass). what is the partial pressure exerted by each gas. attempt at a solution: I know that you need to times the percent of gas in the tank by the pressure. But I try this question so many times keep get me the wrong answer. so please show step by step solution please. I am have a quiz tomorrow so please teach me how to do this problem thanks. 



#2
Oct1407, 10:20 PM

P: 133

This might work: assume 100g total mass sample. Then 92g is CO2, 3.6 g NO etc...
Calculate the mole of each gas with the above masses 92g CO2 = > ? mol CO2 Add up all the moles to get total moles  mole fraction (mol CO2/total moles)is proportional to partial pressure/total pressure,  total pressure is given in the problem. 



#3
Oct1407, 11:40 PM

P: 62

THE ANSWER OF CO2 SHOULD BE 630MM HG 



#4
Oct1507, 12:33 PM

P: 133

Dalton's Law question.
are you sure the % values are correct? If you add up all the numbers I get 100.9%, this could make a difference in the partial pressures




#5
Oct1507, 06:11 PM

P: 62

That's how it is on the book check thousand times!



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