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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 $$\displaystyle { kJmol }^{ -1 }$$:-
259184_994057c8b9a54ac18c389adde0e1ee66.png


A
-7.43
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B
3.72
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C
-3.72
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D
7.43
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Solution

The correct option is A -7.43
heat 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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