ThermochemistryHard
Question
The bond enthalpies of C–C, C=C and C≡C bonds are 348, 610 and 835 kJ/mol, respectively at 298 K and 1 bar. The enthalpy of polymerization per mole of 2-Butyne at 298 K and 1 bar as shown below is
nCH3–C≡C–CH3(g) → –(CH2–CH=CH–CH2)n– (g)
Options
A.−123 kJ
B.−132 kJ
C.−139 kJ
D.−37 kJ
Solution
$\Delta H = \left( \text{B.E}\text{.}_{\pi\text{ bond in C=C}} \right) - \left( \text{B.E}\text{.}_{\sigma\text{ bond in C} - C} \right) = (835 - 610) - 348 = - 123\text{ kJ}$
Create a free account to view solution
View Solution FreeMore Thermochemistry Questions
The standard enthalpy of combustion of solid boron is numerically equal to...The enthalpy of atomization of PH3(g) is +954 kJ/ mol and that of P2H4 is +1.488 MJ/mol. The bond energy of the P–P bond...Heat of neutralisation of CsOH with all strong acid is 13.4 kcal mol-1. The heat released on neutralisation of CsOH with...Determine ᐃUo at 300 K for the following reaction using the listed enthalpies of reaction :4CO(g) + 8H2(g) →...When 1 g equivalent of strong acid reacts with strong base, the heat released is 13.5 kcal. When 1 g equivalent H2A is c...