Home
Class 12
CHEMISTRY
When 1.0 gm of fructose C(6) H(12) O(6) ...

When `1.0` gm of fructose `C_(6) H_(12) O_(6) (s)` is burnt in oxygen in a bomb calorimeter, the temperature of the calorimeter water increases by `1.56^(@)C`. If the heat capacity of the calorimeter and its contents is `10.0 kJ//^(@)C`. Calculate the enthalpy of combustion of fructose at 298 K.

Text Solution

Verified by Experts

Heat capacity of the system
`Delta H_(c) = (-M)/(w) [ C xx overset(uarr) (Deltat)]`
= `(-180)/(1) [ 10 xx 1.56] = -2808 ` kJ/mole
Promotional Banner

Topper's Solved these Questions

  • THERMOCHEMISTRY

    MOTION|Exercise EXERCISE -1 SECTION - A|5 Videos

  • THERMOCHEMISTRY

    MOTION|Exercise EXERCISE -1 SECTION - B|9 Videos

  • SURFACE CHEMISTRY

    MOTION|Exercise Exercise - 3 (Level-II)|12 Videos

  • THERMODYNAMICS

    MOTION|Exercise EXERCISE - 4 (LEVEL - II)|19 Videos

Similar Questions

Explore conceptually related problems

A 1.250 g sample of octane (C_(8)H_(18)) is burned in excess of oxygen in a bomb calorimeter. The temperature of calorimeter rises from 294.05 K to 300.78 K . If heat capacity of the calorimeter is 8.93 kJ K^(-1) , find the heat transferred to calorimeter.

In a calorimeter, the temperature of the calorimeter increases by 6.12 K, the heat capacity of the systemize 1.23 kJ/g deg. What is the molar heat of decomposition for NH_(4)NO_(3) ?

x g sample of NH_(4)NO_(3) is decomposed in a Bomb calorimeter. The temperature of calorimeter increase by 4^(@)C . The heat capacity of the system is 1.25 " kJ"//.^(@)C . Calculate the value of x. Given molar heat of decomposition of NH_(4)NO_(3) at constant volume is 400 kJ " mol"^(-1) .

A sample of CH_(4) of 0.08 g was subjected to combustion at 27^(@)C in a bomb calorimater. The temperature of the calorimeter system was found to be raised by 0.25^(@)C . IF heat capacity of calorimeter is 18K J, Delta H for combustion of CH_(4) at 27^(@)C is