Rate of effusion is inversely proportional to square root of molar mass
rate = k*sqrt(1/M)
M is molar mass
If we take ratio, above expression becomes
rate(SO2)/rate(unknown) = sqrt (M(unknown)/M(SO2))
we have:
M(SO2) = 64.07 g/mol
rate(SO2) = 1.0
rate(unknown) = 2.0
rate(SO2)/rate(unknown) = sqrt (M(unknown)/M(SO2))
1.0/2.0 = sqrt (M(unknown)/64.07)
sqrt (M(unknown)/64.07) = 0.5
(M(unknown)/64.07) = 0.25
M(unknown) = 16.02 g/mol
Molar mass is 16.02 g/mol for CH4
Answer: B
I 22. Which gas would effuse twice as fast as sulfur dioxide (SO2)? Не А. CH4...
I
need help in hurry, please
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Which of the following compounds would you expect to create a
strong electrolyte solution when dissolved in water?
а. СН206 b. SO2 с. ССЦ d. KCl е. F2
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Help?
Q2) In a collision of sufficient force, automobile air bags
respond by electrically triggering the explosive decomposition of
sodium azide (NaN3) to its elements. A 43.398 g sample
of sodium azide was decomposed, and the nitrogen gas generated was
collected over water at 22°C. The total pressure was 798.8 mmHg.
How many liters of dry N2 were generated?
Q3) An atmospheric chemist studying the pollutant SO2
places a mixture of SO2 and O2 in a1.14 L
container at 825.7...
In a collision of sufficient force, automobile air bags respond
by electrically triggering the explosive decomposition of sodium
azide (NaN3) to its elements. A 43.398 g sample of
sodium azide was decomposed, and the nitrogen gas generated was
collected over water at 22°C. The total pressure was 798.8 mmHg.
How many liters of dry N2 were generated?
An atmospheric chemist studying the pollutant SO2
places a mixture of SO2 and O2 in a1.14 L
container at 825.7 K and 2.3...
So i got an 80 and i am not sure which two i got wrong. each
question is worth 10 points. If someone could please help find
which two i got wrong it would be greatly appreciated! I will
rate!
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