Question

# The difference between heats of reaction at constatnt pressure and constant volume for the reaction $$\displaystyle { 2C }_{ 6 }{ H }_{ 6 }\left( l \right) +{ 150 }_{ 2 }\left( g \right) \rightarrow { 12CO }_{ 2 }\left( g \right) +{ 6H }_{ 2 }{ O }\left( l \right) at{ 25 }^{ o }$$ in $$\displaystyle { kJmol }^{ -1 }$$:-

A
-7.43
B
3.72
C
-3.72
D
7.43

Solution

## The correct option is A -7.43heat of reaction at const. pressure $$\displaystyle ={ \Delta }_{ r }H$$heat of reaction at const. pressure $$\displaystyle ={ \Delta }_{ r }U$$$$\displaystyle ={ \Delta }_{ r }H={ \Delta }_{ r }U+{ \Delta }n_{ g }RT$$$$\displaystyle { \Delta }n_{ g }=-3$$$$\displaystyle { \Delta }_{ r }H-{ \Delta }_{ r }U=\left( -3RT \right) =-7432.7 J/mol = -7.432 kJ/mol$$Chemistry

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