Given,
Density of gas = <span>1.653 g/L
Pressure = 746 mm Hg = 0.981 atm
Temperature = 25 degree Celsius or 298 Kelvin
By ideal gas law we know,
PV=nRT
where,
P=Pressure
V=Volume of gas
n= no.of moles
R=Universal gas constant (0.0821)
T= temperature
Now to know the molar mass, we can use following formula;
Molar mass (M) = mass (m)/ no.of moles(n)
or, No.of moles (n)= mass (m)/Molar mass (M)
also, density is related to mass by formula;
Density = Mass(m) * Volume (V)
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Using the above relationship in ideal gas equation, we have,
P.V= m/M. R.T
P. V. M = mRT
M =m /V * RT/P
Since density = m/V, using the relation we get,
M= Density * RT/P
M= (</span>1.653 g/L * 0.082 atm.L/mol.k * 298K)/0.981 atm
<span> = 41.22 g/mol
Hence the molar mass of the gas is 41.22 g/mol
</span>
Answer:
[KI] = 0.25 M
Explanation:
Solute: KI
Mass of solute: 0.50 mol . 166 g / 1mol = 83 g
Our solution volume is 2L
Molarity is a kind of concentration, defined as the moles of solute contained in 1L of solution. It is the most common concentration for all solutions while there are any other kind, for example molality, mole fraction or ppm.
In this case molarity (mol/L) is 0.5 mol /2L = 0.25 M
In conclussion, solution is 0.25 molar whichs is the same to say, that 0.25 moles of potassium iodide are contained in 1L of solution.
With the data given, we can also make a rule of three:
2L of solution contain 0.5 moles of KI
Then, 1L of solution may contain (0.5 . 1) /2 = 0.25 moles of Ki
Answer:
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Explanation:
Answer:
B and C are correct
Explanation:
a) false, pressure increases when volume decreases and temperature increases
b) true, pressure and temperature are directly proportional
c) true, pressure and volume are inversely proportional
d) false, pressure and amount of gas are directly proportional
all of these relations can be summarized by the ideal gas equation:
pV = nRT
p: pressure
V: volume
n: amount of substance
R: gas constant
T: absolute temperature