A: Calculate the mass of nitrogen dissolved at room temperature in an 92.0 L hom
ID: 1022617 • Letter: A
Question
A: Calculate the mass of nitrogen dissolved at room temperature in an 92.0 L home aquarium. Assume a total pressure of 1.0 atm and a mole fraction for nitrogen of 0.78.
Express your answer using two significant figures.
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The following table provides some information on carbon dioxide solubility in water.
Part A
What is the Henry's law constant for CO2 at 20C?
Express your answer to three significant figures and include the appropriate units.
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Part B
What pressure is required to achieve a CO2 concentration of 7.30×102 M at 20C?
Express your answer to three significant figures and include the appropriate units.
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Part C
At 1 atm, how many moles of CO2 are released by raising the temperature of 1 liter of water from 20C to 25C?
Express your answer to four decimal places and include the appropriate units.
C(mol/L) P
(atm) k
(mol/Latm) T
(C) 3.70×102 1.00 20.0 7.30×102 20.0 1.00 3.50×102 25.0
Explanation / Answer
A: Calculate the mass of nitrogen dissolved at room temperature in an 92.0 L home aquarium. Assume a total pressure of 1.0 atm and a mole fraction for nitrogen of 0.78.
Express your answer using two significant figures.
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Use Henry's Law Constant
for N2.
kH= 0.00061 or 6.1x10^-4
x moles initially to convert to grams.
x moles/92.0 L = 0.00061 M/atm * 1 atm
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Multiply both sides by 92.0 L.
Liters and atms will cancelled
x moles = 0.05612moles
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Multiply this by molar mass of N2,
=0.05612moles x 28.02 g/mole= 1.57248g
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Multiply this by mole fraction:
=1.57248g * 0.78 = 1.226g------answer
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