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Formula: C6H6
1 mole of C6H6 produces 6 moles of CO2 during combustion. Therefore, 0.4000 moles of CO2 would require (0.4000 moles CO2) / (6 moles C6H6 per mole CO2) = 0.0667 moles of C6H6 to be completely combusted.
Each molecule of C6H6 contains 6 carbon atoms, so when 1 mole of C6H6 decomposes, 6 moles of carbon atoms are obtained. Therefore, in a 1.68 mole sample of C6H6, 6 × 1.68 = 10.08 moles of carbon atoms can be obtained from the decomposition.
Yes, C6H6 is a hydrocarbon. It is the chemical formula for benzene, which is classified as an aromatic hydrocarbon because it contains a ring structure of carbon atoms with alternating single and double bonds.
C6H6 is an organic compound. Organic compounds are generally carbon-based and contain carbon-hydrogen bonds, such as in benzene (C6H6). Inorganic compounds do not contain carbon-hydrogen bonds.
Formula: C6H6
Benzene has the molecular formula C6H6.
Molar mass C6H6 = 12.0x6 + 1.00x6 = 72 + 6 = 78 g/mole12.7 moles x 78 g/mole = 990.6 grams = 991 g (to 3 significant figures)
cyclohexatriene
There are 3 pi bonds present in benzene (C6H6), which is a cyclic compound with alternating single and double bonds between carbon atoms.
1 mole of C6H6 produces 6 moles of CO2 during combustion. Therefore, 0.4000 moles of CO2 would require (0.4000 moles CO2) / (6 moles C6H6 per mole CO2) = 0.0667 moles of C6H6 to be completely combusted.
Each molecule of C6H6 contains 6 carbon atoms, so when 1 mole of C6H6 decomposes, 6 moles of carbon atoms are obtained. Therefore, in a 1.68 mole sample of C6H6, 6 × 1.68 = 10.08 moles of carbon atoms can be obtained from the decomposition.
the chemical formula is C6H6 that is according to my data
Yes, C6H6 is a hydrocarbon. It is the chemical formula for benzene, which is classified as an aromatic hydrocarbon because it contains a ring structure of carbon atoms with alternating single and double bonds.
C6H6, also known as benzene, consists of 3 pi bonds. These pi bonds are located in the delocalized pi electron cloud above and below the ring of carbon atoms.
To calculate molality, we first need to find the moles of AgClO4 and the moles of solvent, C6H6. Calculate moles of AgClO4: 75.2 g / molar mass of AgClO4 Calculate moles of C6H6: 885 g / molar mass of C6H6 Then, molality (m) = moles of solute / kg of solvent. Divide the moles of AgClO4 by the kg of C6H6 to find the molality of the solution.
Octehedral