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InfinityVicky
02.08.2019 •
Chemistry
Asample of an unknown compound is vaporized at 170 c. the gas produced has a volume of 1980 ml at a pressure of 1 atm, and it weighs 5.17 gr. assuming the gas behaves as an ideal gas under these conditions, calculate the molar mass of the compound. round your answer to 3 significant digits.
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Ответ:
The molar mass is 95.7 g/mol
Explanation:
As the vapor formed is showing ideal gas behavior, it will obey ideal gas law.
PV = nRT
Where
P = Pressure = 1 atm
V = volume = 1980 mL = 1.98 L
n = moles of gas
R = gas constant = 0.0821 L atm /mol K
T = Temperature = 170 °C = 170+273 = 443 K
Putting values
1 X 1.98 = n X 0.0821 X 443
n = moles = 0.054 mol
the relation between moles and molar mass and mass is:
Therefore
Ответ:
Explanation:
A carbon-12 atom has a mass defect of 0.09564 amu. What is its nuclear binding energy? Round to 3 significant figures. x 10 J per carbon-12 atom
First use the formula;
1 amu =934 MeV
therefore 0.09564 will have
934 x 934
= 89.3 MeV