A 0.08468 g sample of gas occupies 10.0-mL at 291.0 K and 1.10 atm. Upon further
ID: 798765 • Letter: A
Question
A 0.08468 g sample of gas occupies 10.0-mL at 291.0 K and 1.10 atm. Upon further analysis, the compound is found to be 13.068% C and 86.932% Br. What is the molecular formula of the compound?Identify the geometry around each carbon atom.
Is this compound polar?
Draw the Lewis structure of the compound.
A 0.08468 g sample of gas occupies 10.0-mL at 291.0 K and 1.10 atm. Upon further analysis, the compound is found to be 13.068% C and 86.932% Br. What is the molecular formula of the compound?
Identify the geometry around each carbon atom.
Is this compound polar?
Draw the Lewis structure of the compound.
A 0.08468 g sample of gas occupies 10.0-mL at 291.0 K and 1.10 atm. Upon further analysis, the compound is found to be 13.068% C and 86.932% Br. What is the molecular formula of the compound?
Identify the geometry around each carbon atom.
Is this compound polar?
Draw the Lewis structure of the compound.
A 0.08468 g sample of gas occupies 10.0-mL at 291.0 K and 1.10 atm. Upon further analysis, the compound is found to be 13.068% C and 86.932% Br. What is the molecular formula of the compound?
Identify the geometry around each carbon atom.
Is this compound polar?
Draw the Lewis structure of the compound.
Identify the geometry around each carbon atom.
Is this compound polar?
Draw the Lewis structure of the compound.
Identify the geometry around each carbon atom. Identify the geometry around each carbon atom. Is this compound polar? Is this compound polar? Is this compound polar? Draw the Lewis structure of the compound. Draw the Lewis structure of the compound. Draw the Lewis structure of the compound.
Explanation / Answer
Use the ideal gas formula to solve for n, because you need the molar mass to find the molecular formula
PV=nRT
n= PV/RT
n= mass/ molar mass
m/MM= PV/RT
MM= m*RT/PV
V= 10ml(1L/ 1000mL)= .01 L
MM= (.08468 g)(.08206)(291)/ (.01*1.1)
MM= 183.8284248 g/mol
Now solve for the emperical formula
mass of C =13.068 g
mass of Br= 86.932 g
moles of C= 13.068g/ 12.0107g/mol= 1.08802984 moles
moles of Br= 86.932g/ (79.904 g/mol)= 1.087955547 moles, Br is smaller amount of moles
moles of C= 1.08802984/1.087955547? 1 mole
moles of Br= 1 mole
Emperical formula= CBr, molecular mass= (12.0107 +79.904)= 91.9147 g/mole
183.8284248/91.9147 = 1.99999?2, 2(CBr)
Molecular Formula = C2Br2
Here is the Lewis structure
The molecular geometry for carbon is going to be linear
The electron pair geometry for carbon is also going to be linear
The compound is nonpolar
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