The molecular mass of a compound is 92 g/mol. Analysis of the compound shows that it consists of 0.608 g of N and 1.388 g of O.
1 answer:
The empirical and molecular formula would be and
respectively.
The compound contains N and O.
N O
0.608/14 = 0.0434 1.388/16 = 0.0867
Divide by the smallest.
N = 1 O = 2
Thus, the empirical formula would be
To get the molecular formula:
Empirical formula mass = 14 + (16x2) = 46
n = molar mass/empirical formula mass
= 92/46 = 2
Thus, the molecular formula would be
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Answer :
(a) The pressure of the vapor in the flask in atm is, 0.989 atm
(b) The temperature of the vapor in the flask in Kelvin is, 372.7 K
The volume of the flask in liters is, 0.2481 L
(c) The mass of vapor present in the flask was, 0.257 g
(d) The number of moles of vapor present are 0.00802 mole.
(e) The mass of one mole of vapor is 32.0 g/mole
Explanation : Given,
Mass of empty flask and stopper = 55.844 g
Volume of liquid = 5 mL
Temperature =
Mass of flask and condensed vapor = 56.101 g
Volume of flask = 248.1 mL
Barometric pressure in the laboratory = 752 mmHg
(a) First we have to determine the pressure of the vapor in the flask in atm.
Pressure of the vapor in the flask = Barometric pressure in the laboratory = 752 mmHg
Conversion used :
or,
As,
So,
Thus, the pressure of the vapor in the flask in atm is, 0.989 atm
(b) Now we have to determine the temperature of the vapor in the flask in Kelvin.
Conversion used :
As,
So,
Thus, the temperature of the vapor in the flask in Kelvin is, 372.7 K
Now we have to determine the volume of the flask in liters.
Conversion used :
1 L = 1000 mL
or,
1 mL = 0.001 L
As, 1 mL = 0.001 L
So, 248.1 mL = 248.1 × 0.001 L = 0.2481 L
Thus, the volume of the flask in liters is, 0.2481 L
(c) Now we have to determine the mass of vapor that was present in the flask.
Mass of flask and condensed vapor = 56.101 g
Mass of empty flask and stopper = 55.844 g
Mass of vapor in flask = Mass of flask and condensed vapor - Mass of empty flask and stopper
Mass of vapor in flask = 56.101 g - 55.844 g
Mass of vapor in flask = 0.257 g
Thus, the mass of vapor present in the flask was, 0.257 g
(d) Now we have to determine the number of moles of vapor present.
Using ideal gas equation:
PV = nRT
where,
P = Pressure of vapor = 0.989 atm
V = Volume of vapor = 0.2481 L
n = number of moles of vapor = ?
R = Gas constant = 0.0821 L.atm/mol.K
T = Temperature of vapor = 372.7 K
Putting values in above equation, we get:
Thus, the number of moles of vapor present are 0.00802 mole.
(e) Now we have to determine the mass of one mole of vapor.
Thus, the mass of one mole of vapor is 32.0 g/mole
The correct IUPAC name of 1,1,1-trimethylheptane is 2,2-dimethyloctane.
<h3>IUPAC NAME:</h3>It is systematic way of nomenclature of organic compounds.
It is based on the position of functional groups, preference of the functional group, long or short chain of carbon, preference of double bond, single and triple bond, branching of carbon chain, etc.
The given compound is 1,1,1-trimethylheptane.
The given name is wrong according to IUPAC name because the numbering of carbon atom should be done in that way in which the carbon atom chain is largest.
Here, in this case the numbering is done from right side. Thus the largest carbon chain have 8 carbon atom.
If the numbering is done according to the question, number of carbon atom in straight chain is 7.
Thus, we concluded that the Correct IUPAC name of 1,1,1-trimethylheptane is 2,2-dimethyloctane.
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<u>True,</u> A mole of one substance has the same number of atoms as a mole of any other substance.
<h3>What is a mole?</h3>
Mole, also spelled mol, in chemistry, a standard scientific unit for measuring large quantities of very small entities such as atoms, molecules, or other specified particles.
The mole designates an extremely large number of units, 6.02214076 × . The General Conference on Weights and Measures defined the mole as this number for the International System of Units (SI) effective from May 20, 2019. The mole was previously defined as the number of atoms determined experimentally to be found in 12 grams of carbon-12.
The number of units in a mole also bears the name Avogadro’s number, or Avogadro’s constant, in honour of the Italian physicist Amedeo Avogadro (1776–1856). Avogadro proposed that equal volumes of gases under the same conditions contain the same number of molecules, a hypothesis that proved useful in determining atomic and molecular weights and which led to the concept of the mole.
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