Home
Class 12
CHEMISTRY
Using the data provided , calculate the ...

Using the data provided , calculate the multiple bond energy `(Kamal^(-1))` of a `C-= C` bond in `C_2H_2` .That energy is ( take the bond energy of a C-H bond as `350 kJ mol^(-1)) .`
`2C(s)+H_2(g)rarrC_2H_2(g)DeltaH=225 kJmol^(-1) `
`2C(s)rarr2C(g)DeltaH=1410kJmol^(-1)`
`H_2(g)rarr2H(g)DeltaH=330 kJmol^(-1)`

A

`1165`

B

`837`

C

`865`

D

`815`

Text Solution

Verified by Experts

The correct Answer is:
D
`therefore " " DeltaH = +1410 + 330 -(350 xx 2) - epsilon _(C-=C) = 1740 - 700 - 225=+ 815` KJ/mol.
Promotional Banner

Topper's Solved these Questions

  • THERMODYNAMICS

    RESONANCE ENGLISH|Exercise exercise-3 Part-2 :(previous years)|11 Videos

  • THERMODYNAMICS

    RESONANCE ENGLISH|Exercise exercise-3 Part-3 :(Subjective questions)|6 Videos

  • THERMODYNAMICS

    RESONANCE ENGLISH|Exercise exercise-2 Part-4 : Comprehension|5 Videos

  • TEST SERIES

    RESONANCE ENGLISH|Exercise CHEMISTRY|50 Videos

Similar Questions

Explore conceptually related problems

Using the data provided, calculate the multiple bond energy (kJ mol^(-1)) of a C-=C bond in C_(2)H_(2) . That energy is ( take the bond energy of a C-H bond as 350kJ mol^(-1)) . 2C_((s))+H_(2(g))rarr C_(2)H_(2(g)), Delta=225kJ mol^(-1) 2C_((s))rarr 2C_(g)), DeltaH=1410kJ mol^(-1) H_(2(g)) rarr 2H_((g)),DeltaH=330kJ mol^(-1)

The average O-H bond energy in H_(2)O with the help of following data. (1) H_(2)O(l)rarrH_(2)O(g), Delta H= +40.6 kJ mol^(-1) (2) 2H(g)rarrH_(2)(g), DeltaH= -435.kJ mol^(-1) (3) O_(2)(g)rarr2O(g), Delta H= +489.6 kJ mol^(-1) (4) 2H_(2)(g)+O_(2)(g)rarr2H_(2)O(l), Delta H= -571.6 kJ mol^(-1)

The H-H bond energy is 430KJmol^(-1) and Cl-Cl bond energy is 240KJmol^(-1) . DeltaH for HCl is -90KJ . The H-Cl bond energy is about

The enthalpy change for the reaction, C_(2)H_(6)(g)rarr2C(g)+6H(g) is X kJ. The bond energy of C-H bond is :

Calculate DeltaH^(@) ("in" kJmol^(-1)) for the reaction CH_(2)Cl_(2)(g)rarrC(g)+2H(g)+2Cl(g). The average bond enthalpie of C-H and C-C1 bonds are 414 kJ mol^(-1) .

The enthalpy changes at 298 K in successive breaking of O-H bonds of water, are H_(2)O(g) rarr H(g)+OH(g),DeltaH=498kJ mol^(-1) OH(g) rarr H(g)+O(g), DeltaH =428 kJ mol^(-1) The bond energy of the O-H bond is

The dissociation energy of CH_(4)(g) is 360 kcal mol^(-1) and that of C_(2)H_(6)(g) is 620 kcal mol^(-1) . The C-C bond energy

Find the bond energy of S-S bond from the following data: {:(C_(2)H_(5)-S-C_(2)H_(5)(g),,,,Delta_(f)H^(@)=-147KJmol^(-1)),(C_(2)H_(5)-S-S-C_(2)H_(5)(g),,,,Delta_(f)H^(@)=-201KJmol^(-1)),(S(g),,,,Delta_(f)H^(@)=222 KJ mol^(-1)):}

From the following bond energies :- H-H "bond energy" = 420 KJmol^(-1) C-=C "bond energy" = 601 KJmol^(-1) C-C "bond energy"=340KJmol^(-1) C-H "bond energy" = 425 KJ mol^(-1) Enthalpy for the reaction :- C_(2)H_(2)+2H_(2)toC_(2)H_(6)

Find bond enthalpy of S-S bond from the following data: C_(2)H_(5)-S-C_(2)H_(5)," "DeltaH_(f)^(@)=-147.2kJ" "mol^(-1) C_(2)H_(5)-S-S-C_(2)H_(5)," "DeltaH_(f)^(@)=-201.9kJ" "mol^(-1) S(g)," "DeltaH_(f)^(@)=222.8kJ" "mol^(-1)