Home
Class 12
CHEMISTRY
For the complete combustion of ethanol, ...

For the complete combustion of ethanol, `C_(2)H_(5)OH(l)+3O_(2)(g)rarr2CO_(2)(g)+3H_(2)O(l)` the amount of heat produced as measured in bomb calorimeter is `1364.47KJ mol^(-1)` at `25^(@)C` . Assuming ideality, the enthalpy of combustion, `DeltaH_(C)` , for the reaction will be
`[R=8.314JK^(-1)mol^(-1)]`

A

`-1460.50 kJ mol^(-1)`

B

`-1350.50 kJ mol^(-1)`

C

`-1366.95 kJ mol^(-1)`

D

`-1361.95 kJ mol^(-1)`

Text Solution

AI Generated Solution

Doubtnut Promotions Banner Mobile Dark
|

Topper's Solved these Questions

  • JEE MAINS

    JEE MAINS PREVIOUS YEAR ENGLISH|Exercise QUESTION|1 Videos

  • JEE MAIN

    JEE MAINS PREVIOUS YEAR ENGLISH|Exercise CHEMISTRY|146 Videos

  • JEE MAINS 2020

    JEE MAINS PREVIOUS YEAR ENGLISH|Exercise CHEMSITRY|23 Videos

Similar Questions

Explore conceptually related problems

For the reaction C_(3)H_(8)(g)+5O_(2)(g)rarr3CO_(2)(g)+4H_(2)O(l) at constant temperature, DeltaH-DeltaU is

For the reaction : C_(2)H_(5)OH(l)+3O_(2)(g)rarr2CO_(2)(g)+3H_(2)O(g) if Delta U^(@)= -1373 kJ mol^(-1) at 298 K . Calculate Delta H^(@)

Knowledge Check

  • The combustion of benzene(/) gives CO_2(g) and H_2O(l) Given that heat of combustion of benzene at constant volume is -3263.9 kJ mol^(-1) at 25^@C , heat of combustion (in kJ mol^(-1) ) of benzene at constant pressure will be (R = 8.314 JK^(-1) mol^(-1))

    A
    `4152.6`
    B
    `-452.46`
    C
    `3260`
    D
    `-3267.6`

    • Similar Questions

    Explore conceptually related problems

    For the reaction, C_(7)H_(8)(I) + 9O_(2)(g) rarr 7 CO_(2)(g) + 4H_(2)O(I) , the calculated heat of reaction is 232 kJ mol^(-1) and observed heat of reaction is 50.4 kJ mol^(-1) , then the resonance energy is

    The combustion of benzene (l) gives CO_(2)(g) and H_(2)O(l) . Given that heat of combustion of benzene at constant volume is –3263.9 kJ mol^(–1) at 25^(@)C , heat of combustion (in kJ mol^(–1) ) of benzene at constant pressure will be (R = 8.314 JK–1 mol–1)

    The reaction: NH_(2)CN(s) +(3)/(2)O_(2)(g)rarr N_(2)(g) +CO_(2)(g) +H_(2)O(l) Was carried out in a bomb caloriemeter. The heat released was 743 kJ mol^(-1) . The value of DeltaH_(300K) for this reaction would be

    C_(4)H_(10)+(13)/(2)O_(2)(g)rarr4CO_(2)(g)+5H_(2)O(l), DeltaH =- 2878 kJ DeltaH is the heat of……….of butane gas.

    Balance chemical equation is given as following: C_(2)H_(5)OH(l)+3O_(2)(g) rarr 2CO_(2)(g)+3H_(2)O(l) What value of the volume in litre of CO_(2) (g) measured at 200 K and 1 atm, produced from the combustion of 0.25 mole of C_(2)H_(5)OH (l) / [Use R = 0.08 L "atm mol"^(-1) K^(-1) ]

    Consider the reacting at 300K C_(6)H_(6)(l)+(15)/(2)O_(2)(l)rarr 6CO_(2)(g)+3H_(2)O(l),DeltaH=-3271 kJ What is DeltaU for the combustion of 1.5 mole of benzene at 27^(@)C ?

    Calculate the heat of combustion of eithene CH_(2) = CH_(2)(g) + 3O_(2)(g) rarr 2CO_(2)(g) + 2H_(2)O(I) The bond energy data are given below C = C = 619 kJ mol^(-1) C - H = 414 kJ mol^(-1) O = O = 499 kJ mol^(-1) C = O = 724 kJ mol^(-1) O - H = 460 kJ mol^(-1)

    Home
    Profile