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Difference between the heats of reaction...

Difference between the heats of reaction at constant pressure and a constant volume for the reaction `2C_(6)H_(6)(l) + 15O_(2)(g) rarr 12CO_(2)(g) + 6H_(2)O(l)` at `25^(@)C` in `kJ` is

A

`-7.43`

B

`+3.72`

C

`-3.72`

D

`+7.43`

Text Solution

AI Generated Solution

To find the difference between the heats of reaction at constant pressure (\( \Delta H \)) and constant volume (\( \Delta U \)) for the reaction: \[ 2C_{6}H_{6}(l) + 15O_{2}(g) \rightarrow 12CO_{2}(g) + 6H_{2}O(l) \] at \( 25^\circ C \), we can follow these steps: ### Step 1: Identify the reaction and the number of moles of gaseous products and reactants. ...
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Calculate the difference between the heats of reaction at constant pressure and constant volume for the reaction 2C_6H_6(l) + 15O_2(g) to 12CO_2(g) + 6H_2O (l) at 25^@C in kJ.

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Knowledge Check

  • The difference between heats of reaction at constant pressure and constant volume for the reaction, 2C_6H_6(l) + 15O_2(g) to 12CO_2(g) + 6H_2O (l) at 25^@C in kJ is

    A
    ` + 7.43`
    B
    ` +3.72`
    C
    `-7.43`
    D
    `-3.72`

  • For combustion of 1 mole of benzene at 25^(@)C , the heat of reaction at constant pressure is -780.9" kcal." What will be the heat of reaction at constant volume ? C_(6)H_(6(l))+7(1)/(2)O_(2(g))rarr 6CO_(2(g))+3H_(2)O_((l))

    A
    `-781.8" kcal"`
    B
    `-"780.0 kcal"`
    C
    `+"781.8 kcal"`
    D
    `+"780.0 kcal"`

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