Which of the following woud you expect to have a higher boiling point? Why?
1. CH4 or HF
2. CH3OCH3 CH3CH2OH
3. CH4 of C2H6
4. CH4 or SiH4
Case 1) Methane is gas and boils at -161 °C and HF boiling point is 19.5 °C. Due strong intra molecular hydrogen bondings of HF, HF has higher boining point compare to methane.
Case 2) Di ethyl ether has less boing point (34 °C) as compare to ethanol (64 °C), due to same reason as above of intra molecular hydrogen bonding.
Case 3) Methane is gas at room temperature as discussed earlier and boils at -161°C, benzene is liquid and boils at 80 °C. Due to Pi bond attraction within the molecules make it higher boing as compare to methane.
Case 4) Here Metane and Silane (-112 °) and both volatile, but silane is more polar character as compare to methane and due to its high molecular weight it has higher boiling point as compare to methane.
Which of the following woud you expect to have a higher boiling point? Why? 1. CH4...
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please help Which of the following would you expect to have the higher boiling point? WHY? H 1 H : Br: H LH or sc H N: C C HH Br: innoint? In your answer explain
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