Both of these compounds are alkanes with four carbon atoms and both of these compounds have the molecular formula C4H10. These are structural isomers of each other.
the molar mass!!
The melting and boiling points are different. Butane has a melting point of 135.4K and 2-methylpropane [isobutane] has a melting point of 114K. The boiling point of Butane is 272.6K and isobutane @ 261K. It has to do with there structures. J
1-bromobutane 2-bromobutane 1-bromo 2-methylpropane 2-bromo 2-methylpropane
Butane has 2 isomers:CH3CH2CH2CH3 - butaneCH3CH(CH3)CH3 - 2-methylpropane (or isobutane)
The molecule of Methane is CH4; 1 carbon and 4 hydrogen atoms Butane's molecule C4H10 has 4 Carbon atoms and 10 hydrogen. So Butane has more parts to burn (connect to oxygen/oxidise) per molecule, hence a higher calorific value.
There are two structural isomers approved by IUPAC (International Union of Pure and Applied Chemistry) 1.) n-butane (normal butane) is a straight chain 2.) iso-butane (or methyl-propane) is a chain of three with one carbon attached to the middle of the chain
The melting and boiling points are different. Butane has a melting point of 135.4K and 2-methylpropane [isobutane] has a melting point of 114K. The boiling point of Butane is 272.6K and isobutane @ 261K. It has to do with there structures. J
1-bromobutane 2-bromobutane 1-bromo 2-methylpropane 2-bromo 2-methylpropane
Yes
Butane has higher melting and boiling points.
There's no such molecule; elements cannot combine that way. If you meant H10C4, then it's a structural isomer of butane. (Butane or 2-methylpropane.)
Only two isomers are possible 1,Butane and 2, 2-methyl propane. Not quite: "butane" has no need for a number and the second compound should be simply "2-methylpropane" or even more simply "methylpropane" since there is only one possible structure for it.
Ch3ch3cclch3
Butane has 2 isomers:CH3CH2CH2CH3 - butaneCH3CH(CH3)CH3 - 2-methylpropane (or isobutane)
The molecule of Methane is CH4; 1 carbon and 4 hydrogen atoms Butane's molecule C4H10 has 4 Carbon atoms and 10 hydrogen. So Butane has more parts to burn (connect to oxygen/oxidise) per molecule, hence a higher calorific value.
There are two structural isomers approved by IUPAC (International Union of Pure and Applied Chemistry) 1.) n-butane (normal butane) is a straight chain 2.) iso-butane (or methyl-propane) is a chain of three with one carbon attached to the middle of the chain
butane density
n-butane : Melting point −138.4 °C (135.4 K), boiling at −0.5 °C (272.6 K)iso-butane (methylpropane): Melting point -159.6 °C, (114 K) , boiling at -11.7 °C, (261 K)