CameraIcon
CameraIcon
SearchIcon
MyQuestionIcon


Question

Heat of a reaction is defined as the amount of heat absorbed or evolved at a given temperature when the reactants have combined to form the products is represented by balanced chemical equation. If the heat is denoted by q then the numerical value of q depends on the manner in which
the reaction is performed for two methods of conducting chemical reactions in calorimeters.

The heat of combustion of maltose at a constant volume in the above question if water vapour is not condensed will be:


A
-1350 kcal/mol
loader
B
-1343 kcal/mol
loader
C
-1370 kcal/mol
loader
D
-1400 kcal/mol
loader

Solution

The correct option is B -1343 kcal/mol
 q=ΔE+PΔV  or q=ΔE+ΔngRT
where ΔE= the heat of combustion in calorimeteric bomb.
Reaction:
C12H22O11(s)+12O2(g)12CO2(g)+11H2O(g)
On putting values we get
q=1350+11×2×29810001343 kcal/mol

Chemistry

Suggest Corrections
thumbs-up
 
0


similar_icon
Similar questions
View More


similar_icon
People also searched for
View More



footer-image