Butanol has the chemical formula C4H9OH. a) Show the full electron configuration for C and indicate how many electrons C needs to have a full valence shell. b) Butanol has a density of 810 kg m-3. How many molecules of butane are there in 150 mL? c) Butanol and oxygen react in a combustion reaction with the formula below. Balance the formula and determine how many moles of CO2 are produced from 2.5 mol of butane C4H9OH (l) + O2 (g) CO2 (g) + H2O (l)
Butanol has the chemical formula C4H9OH.
a) Show the full electron configuration for C and indicate how many electrons C needs to have a full valence shell.
b) Butanol has a density of 810 kg m-3. How many molecules of butane are there in 150 mL?
c) Butanol and oxygen react in a combustion reaction with the formula below. Balance the formula and determine how many moles of CO2 are produced from 2.5 mol of butane
C4H9OH (l) + O2 (g) CO2 (g) + H2O (l)
d) In the molecule of butanol, there are C-C bonds, C-H bonds, a C-O bond and a O-H bond. Order these bonds from most to least polar
e) On average, would you expect C-C to have longer or shorter bonds than C-H Briefly explain your answer.
f) From the reaction 2.57 L of carbon dioxide was produced and captured. Calculate the number of molecules of carbon dioxide if the temperature was 25.0 C and the pressure 1. 01 × 105 Pa.
g) The empirical and molecular formula for butanol is the same. Briefly explain why.
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