Home
Class 11
CHEMISTRY
The bond energy (in kcal mol^(-1)) of a ...

The bond energy (in kcal `mol^(-1))` of a `C -c` single bond is approximately

A

`1`

B

`10`

C

`100`

D

`1000`

Text Solution

AI Generated Solution

To determine the bond energy of a carbon-carbon (C-C) single bond, we can follow these steps: ### Step-by-Step Solution: 1. **Understanding Bond Energy**: - Bond energy, also known as bond dissociation energy, is the amount of energy required to break a bond between two atoms in a molecule. For a C-C single bond, this energy is needed to separate the two carbon atoms completely. 2. **Identifying the Nature of the Process**: ...
Doubtnut Promotions Banner Mobile Dark
|

Topper's Solved these Questions

  • THERMODYNAMICS

    CENGAGE CHEMISTRY|Exercise Archives (Assertion-Reasoning)|3 Videos

  • THERMODYNAMICS

    CENGAGE CHEMISTRY|Exercise Archives (Interger)|1 Videos

  • THERMODYNAMICS

    CENGAGE CHEMISTRY|Exercise Archives (Multiple Correct)|3 Videos

  • STOICHIOMETRY

    CENGAGE CHEMISTRY|Exercise Archives Subjective|33 Videos

Similar Questions

Explore conceptually related problems

The average energy required to break a P-P bond in P_(4)(s) into gaseous atoms is 53.2 kcal mol^(-1) . The bond dissociation energy of H_(2)(g) is 104.2kcal mol^(-1) , Delta H_(f)^(0) of PH_(3)(g) from P_(4)(s) is 5.5 kcal mol^(-1) . The P-H bond energy in kcal mol^(-1) is [ Neglect presence of Van der Waals force in P_(4)(s) ]

Using the data provided, calculate the bond energy ( kJ mol^(-1)) of a C-=C bond in C_(2)H_(2) . That eneergy is ( take the bond energy ofC-H bond as350 kJ mol^(-1)) 2C(s) + H_(2)(g) rarr C_(2)H_(2)(g)" " DeltaH = 225 kJ mol^(-1) 2C(s) rarr 2C(g) " " DeltaH = 1410 kJ mol^(-1) H_(2)(g) rarr 2H(g)" " DeltaH = 330 kJ mol^(-1)

Knowledge Check

  • The bond energy (in Kcal mol^(-) ) of a C-C single bond is approximately:

    A
    `1`
    B
    `10`
    C
    `100`
    D
    `1000`

  • 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 350 kJ mol^(-1)) 2 C (s) + H_(2) (g) to C_(2) H_(2) (g) Delta H = 225 k J mol^(-1) 2 C (s) to 2 C (g) " " Delta H = 1410 kJ mol^(-1) H_(2) (g) to 2 H (g) " " Delta H = 330 kJ mol^(-1)

    A
    1165
    B
    837
    C
    865
    D
    815

  • The catenation tendency of C, Si , and Ge is in the order Ge lt Si lt C . The bond energies (in kJ mol^(-1) ) of C-C-, Si-Si , and Ge-Ge bonds, respectively, are

    A
    `167, 180, 348`
    B
    `180, 167, 348`
    C
    `348, 167, 180`
    D
    `398, 180, 167`

    • Similar Questions

    Explore conceptually related problems

    The bond energy of H_(2) is 104.3 kcal mol^(-1) . If means that :

    The bond energy of C-C bond in Kcal/mol is -

    The bond energy of H_(2) is 104.3 k.cal mol^(-1) . It means that

    The enthalpy of formation of UF(g) is 22kcal mol^(-1) and that of U(g) is 128kcal mol^(-1) . The bond energy of the F-F bond is 37kcal mol^(-1) . The bond dissociation energy of UF(g) is (are):

    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 350 kJ mol^(-1) ) 2C(s)+H_(2)(g)rarrC_(2)H_(2)(g)" "DeltaH=225 kJ mol^(-1) 2C(s)rarr2C(g)" "DeltaH=1410kJ mol^(-1) H_(2)(g)rarr2H(g)" "DeltaH=330kJ mol^(-1)

    Home
    Profile